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Keywords:

  • methanol;
  • OVOC;
  • oxygenated hydrocarbons;
  • atmosphere;
  • ocean

Abstract

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[1] Methanol is a biogeochemically active compound and a significant component of the volatile organic carbon in the atmosphere. It influences background tropospheric photochemistry and may serve as a tracer for biogenic emissions. The mass of methanol in the atmospheric reservoir, the annual mass flux of methanol from sources to sinks, and the estimated atmospheric lifetime of methanol in the free troposphere, marine boundary layer, continental boundary layer, and in-cloud, are evaluated. The atmosphere contains approximately 4 Tg (terragrams, 1012 g) of methanol. Estimates of global methanol sources and sinks total 340 and 270 Tg methanol yr−1, respectively, and are in balance given their estimated precision. Sink terms were evaluated using observed methanol distributions; the total loss is approximately a factor of 5 larger than prior estimates. The adopted source is a factor of 3 larger than its prior estimate. Recent net flux observations and the magnitude of the estimated sink suggest biogenic methanol emissions to be near their current estimated upper limit, >280 Tg methanol yr−1, and this value was adopted. The methanol source will be larger with the inclusion of an argued for oceanic gross emission of 30 Tg methanol yr−1, but a major uncertainty concerns whether the oceans are a major net sink or source of methanol, an issue which will not be resolved without new measurements. Other large uncertainties are the estimates of primary biogenic emissions and gas surface deposition. The first loss estimates of methanol by in-cloud chemistry and precipitation are presented. They are approximately equal at 10 Tg methanol yr−1, each. These are small in comparison to the surface loss and gas phase photochemical loss estimated here but would be significant additional losses in earlier budgets. Surface exchange processes dominate the atmospheric budget of methanol and its distribution. The atmospheric deposition of methanol and the argued for methanol produced in the upper ocean are ubiquitous sources of C1 substrate capable of sustaining methylotrophic organisms throughout the surface ocean.

1. Introduction

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[2] Methanol is the predominant oxygenated organic compound in the background mid to upper troposphere [Singh et al., 2000, 2001]. Methanol emissions represent approximately 6% of identified terrestrial biogenic organic carbon sources to the atmosphere based upon the data in Fall [1999] and this work (Table 1). For comparison, global methanol sources, on a carbon mass basis, may be a factor of 2 larger than those inferred by Jacob et al. [2002] for acetone. The atmospheric lifetime of methanol due to the reaction with gaseous HO alone is on the order of 19 days, based on observed methanol distributions and predicted HO fields from the global photochemical model of Bey et al. [2001]. Consequently, methanol is transported globally [e.g., Singh et al., 2001] and is proposed to have a role in tropospheric oxidant photochemistry [e.g., Fehsenfeld et al., 1992; Kelly et al., 1994; Monod et al., 2000]. Additionally, methanol could serve as an intermediate-lived atmospheric tracer of terrestrial biogenic emissions, as it is emitted from a variety of plant species [Fall and Benson, 1996], although its efficacy as a tracer would be reduced should oceanic emissions prove to be significant.

Table 1. Estimated Biogenic Emissions of Volatile Organic Compounds, Tg-C yr−1a
SpeciesMinimumMaximumMidvaluePercentage
Methane31941236623
Isoprene17550333922
Monoterpene family12748030419
Dimethylsulfide1530231
Ethylene825171
Other reactive VOC's  26017
Other less reactive VOC's  26017
Total VOC  1567100
Biogenic methanolb  1006
Total Methanolb  128 
Total Acetonec  59 

[3] Methanol directly reacts with hydroxyl radicals (HO) in gas and aqueous phases. The reaction products are a subsequent source of formaldehyde, hydrogen radicals, and ozone. In addition, methanol photochemistry in cloud water can be a source of formic acid [e.g., Jacob, 1986, 2000]; and it therefore has a potential role in establishing the background acidity of cloud and rainwater. In-cloud methanol chemistry confounds the prediction of cloud effects on, for example, atmospheric ozone, formaldehyde, carbon monoxide, and molecular hydrogen [Lelieveld and Crutzen, 1991; Jacob, 2000; Monod et al., 2000]. The methanol photochemical lifetime is long compared to formaldehyde (∼1 day), and methylhydroperoxide (1–2 days); the predominant oxygenated organic compounds in the lower troposphere especially over continents. Methanol lifetime in the surface boundary layer is 3–6 days and in cloud it is 9 days. Quantification of methanol distributions, the global sinks of methanol, and its global sources is needed before the significance of methanol on tropospheric photochemistry can be accurately determined.

[4] Measurements of methanol in the near surface atmosphere, though limited in number, show a consistent range of values within general land use types (Table 2a). Most of the data are from spring-summer measurement campaigns during vegetative growth stages and seasonal information from single locales is sparse. Typical methanol surface concentrations are estimated at 900 pptv (pptv is defined as 1012 times the molecular mixing ratio of methanol in air) over the remote ocean, 2000 pptv for continental background, 6000 pptv for grasslands, 10000 pptv for coniferous and deciduous forests, and >20000 pptv for urban areas. Kelly et al. [1993] report three extreme observations (78,500, 212,000, and 297,000 pptv) in a wooded North Carolina industrial area. Isolated methanol observations in the Arctic have been reported during summer by Cavanagh et al. [1969] and during polar sunrise by Boudries et al. [2002] with mean values nominally 800 and 250 pptv, respectively. The mean methanol concentration for four Arizona rainwater samples from Snider and Dawson [1985] is also listed: the only rainwater observations available. Estimates of methanol concentrations in atmospheric water are also given assuming gas-aqueous thermodynamic equilibrium, Henrys' Law data from Snider and Dawson [1985], and the typical gas concentrations stated above. Atmospheric water concentrations are predicted to range from 0.2 to >4 × 10−6 M for 25°C, or from 0.9 to >20 × 10−6 M for 0°C along a gradient from background ocean to urban conditions.

Table 2a. Atmospheric Methanol Observations
Measurement/EstimateMean ValueRangeReference
Near-Surface, ppt
Arctic (2/14–3/10; Alert, Nunavut, Canada)20041–42424 hr. no sun, Boudries et al. [2002]
Arctic (3/10–31; Alert, Nunavut, Canada)26942–571Transition, Boudries et al. [2002]
Arctic (4/1–5/1; Alert, Nunavut, Canada)25634–59424 hr. sun, Boudries et al. [2002]
Remote ocean (Pacific and N. Atlantic)900200–1200Singh et al. [2000, 2001]
Hayfield (Austria)60004000–9000Karl et al. [2001]
Urban (Innsbruck Austria)750030–45000Holzinger et al. [2001]
Tropical rain forest (Surinam)1100 Williams et al [2001]
Urban (San Paulo, Rio de Janeiro, and Salvador, Brazil) <7600–72000de Paula Pereira et al. [1999]
Aged urban and pine forest day (Calif.)100004000–10000Lamanna and Goldstein [1999]
Boundary layer forest (Mass.)200005000–37000Doskey and Gao [1999]
Rural/forest/field/urban (Tenn.)110003000–22000Riemer et al. [1998]
Mountain background (Colo.)20002000–4000Goldan et al. [1997]
Urban/mountain upsloe (Colo.)60003000–6000Goldan et al. [1997]
Rural (Garm.-Part. Germany)23001200–4000Leibrock and Slemr [1997]
Urban (Kuwait), 4 sites5500043000–65000Bouhamra [1996]
Rural (Kuwait), 2 sites100040–1900Bouhamra [1996]
Urban (Colo.)200001000–17000Goldan et al. [1995a]
Background estimate (Colo.)20001900 + 0.17*[NOy]Goldan et al. [1995a]
Fresh urban estimate (Colo.)200001900 + 0.17*[NOy]Goldan et al. [1995a]
Rural forest day (Ala.)110001000–20000Goldan et al. [1995b]
Rural forest night (Ala.)60001000–20000Goldan et al. [1995b]
Urban (Boston, Mass.)174007200–47000Kelly et al. [1993]
Urban (Houston, Tex.)166005600–31000Kelly et al. [1993]
Industrial area (N. C.), 3 samples19500078500–297000Kelly et al. [1993]
Rural (AZ)2600±1100Snider and Dawson [1985]
Urban (AZ)7900±2600Snider and Dawson [1985]
Arctic (summer, Pt. Barrow, Alaska)800400–1200Cavanagh et al. [1969]
 
Troposphere Aloft, ppt
Alps (Sonnblick, Austria), 3.1 km12501000–5000T. Karl (personal communication, 2002)
Remote ocean, (Pac. and N. Atl.) 2–12 km600300–1200Singh et al. [1995, 2000, 2001]
Tropical (Surinam)600 Williams et al. [2001]
New England forest (MA), 1–3 km200005000–15000Doskey and Gao [1999]
Rocky Mountains (CO), ∼3 km2000 Goldan et al. [1997]
Mauna Loa Observatory (HI), ∼3km 500–2000T. Karl (personal communication)
 
Rain, Nano-Molar
Rural (AZ)690 Snider and Dawson [1985]

[5] Methanol observations aloft are few. Singh et al. [1995, 2000, 2001] have reported values for the remote atmosphere over the Atlantic and Pacific from 0.3 to 12 km. Mixing ratios between 200 and 1000 pptv were shown and 600 pptv is estimated as a central value for the free troposphere (FT). Doskey and Gao [1999] showed lower tropospheric methanol observations near the top of the boundary layer over Harvard Forest, MA, and these ranged from 5000–15000 pptv and were approximately equation image those measured near the surface. Mountain site data from Colorado suggest background concentrations of 2000 pptv [Goldan et al., 1997] in the lower continental troposphere. T. Karl (personal communication, 2002) has data from a Colorado mountain site showing similar values. He also has data, which range from 500–2000 pptv for Mauna Loa Observatory (MLO), HI. MLO is at approxately 3 km altitude, is subject to strong upslope-downslope flow, and mixing ratios there reflect at times lower FT air, island modified MBL air, or a mixture of these air mass types. Williams et al. [2001] reported methanol from the initial airborne deployment of a proton transfer reaction mass spectrometer. Their measurements were in the tropics over Surinam during March and mean FT(>3 km) and lower-FT (<3 km) mixing ratios were 600 and 1100 ppt, respectively. The latter value is low compared with other midlatitude continental observations.

[6] The present atmospheric budget of methanol is poorly constrained [Singh et al., 2000, 2001] and is the subject of this work. Singh et al. [2000] estimated the total atmospheric methanol source at 122 Tg methanol with fossil-fuel combustion (3 Tg methanol yr−1), terrestrial primary biogenic emissions (75 Tg methanol yr−1), methane oxidation (18 Tg methanol yr−1), terrestrial biomass decay (20 Tg methanol yr−1), and biomass burning (6 Tg methanol yr−1) considered separately. An oceanic source was suggested but without a value given. Their combined sources exceeded the sum of the two methanol sinks considered, 40–50 Tg methanol yr−1, by a factor of 2 to 3. This discrepancy motivated a more critical examination of other methanol sinks (section 2) including precipitation removal and in-cloud chemistry, as well as, a reassessment of losses by surface gas deposition and HO reaction. We used observed mixing ratios to estimate loss rates in our analysis and found our new combined sink exceeded their source estimate by about 2.5. The newfound excess in global loss prompted a reconsideration of sources (section 3) principally the primary terrestrial biogenic source with the inclusion of recent net flux studies (section 4) and an evaluation of a possible oceanic source. Table 3 summarizes the data used to establish the primary terrestrial biogenic source of methanol. Table 4 presents a revised budget for atmospheric methanol based on this effort. The budget is presented in units of Tg methanol (terragrams of methanol) for consistency with the earlier Singh et al. budget. Table 4 includes a hypothesized but untested oceanic source of methanol. Table 5 summarizes phytoplankton culture work in support of this hypothesis. While this work strives to develop methanol budget closure, it calls out the uncertainty in global source and sink terms.

2. Methanol Sinks Considered

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[7] There are no studies quantifying methanol loss on a global basis aside from that of Singh et al. [2000], wherein they considered two methanol sink processes: gas phase hydroxyl radical (HO) reaction and surface deposition (uniform global deposition velocity, Vs, of 0.1 cm s−1). These and other methanol loss processes including consumption by leaf microbes, precipitation, dew, and atmospheric vertical transport and mixing, have been identified to explain daily cycles and rapid changes in methanol concentrations observed in surface time series [e.g., Snider and Dawson, 1985; Goldan et al., 1995a, 1995b, 1997; Fall, 1996; Leibrock and Slemr, 1997; Doskey and Gao, 1999; Riemer et al., 1998]. An in-cloud loss by the aqueous reaction of methanol with HO can be added to this list based on the work of Jacob [1986], Lelieveld and Crutzen [1991], and Monod and Carlier [1999]. The following is an initial global analysis of methanol loss by aqueous methanol-HO reaction in cloud and precipitation deposition to land and ocean. These are followed by reanalyses of its losses through “dry” deposition to land and ocean and methanol-HO reaction in the gas phase. Such estimates have necessarily large variances and these are included in Table 4. The sink terms are evaluated using observed atmospheric mixing ratios.

2.1. Aqueous Phase HO Reaction

[8] Methanol loss by reaction with HO can occur in the gas phase and in the aqueous phase within atmospheric water (e.g., haze aerosol, clouds, fog, rain). In cloud aqueous reactions of methanol have been discussed as they pertain to HO, formaldehyde, and ozone chemistry [e.g., Monod and Carlier, 1999; Jacob, 2000; Monod et al., 2000], but not as a sink of methanol. A simple calculation illustrates the potential for loss of methanol by aqueous HO chemistry in oceanic and continental water clouds. The overall aqueous reaction is:

  • equation image

The reaction rate constant is 1 × 109 M−1 s−1 and estimated from Monod and Carlier [1999]. A HO value of 0.1 × 10−12 M was used to estimate a minimum cloud loss rate based on work by Jacob [1986, 2000]. Gas-aqueous thermodynamic equilibrium is assumed to estimate maximum aqueous HO and to estimate methanol concentrations from their gas phase concentrations. For maximum HO, the global mean HO concentration of 1 × 106 molecules cm−3 [Prinn et al., 1995] is used. This must be reduced by about 50% to account for in-cloud photochemical conditions [Jacob, 2000]. The HO Henry's Law constant is 100 M atm−1 (Tcloud = 0°C [Jacob, 2000]). This is reduced by 80% to account for kinetic gas-to-droplet mass transfer limitations [Jacob, 1986], as HO reacts with many dissolved species in cloud water such that gas-droplet mass transfer of HO is unable to sustain aqueous concentrations near the thermodynamic equilibrium value. Jacob [1986] modeled in-cloud aqueous and gas phase HO concentrations as a function of droplet pH at 293°K and the aqueous-to-gas ratio at pH = 5 was 4 M atm−1 which is about 20% of that expected from thermodynamic equilibrium. The resultant maximum aqueous HO concentration is then 0.4 × 10−12 M. A background gas phase methanol concentration of 900 pptv (Table 2b) was used for oceanic clouds and 2000 pptv (Table 2b) was used for continental clouds. The methanol Henry's Law constant is 1000 M atm−1 (Tcloud = 0°C [Snider and Dawson, 1985]). Resulting aqueous methanol concentrations are 2 × 10−6 M and 9 × 10−7 M for continental and oceanic clouds, respectively. The oceanic and continental cloud liquid water content was set to 3 × 10−7 L/L based upon values given by Lelieveld and Crutzen [1991]. Cloud volumes were estimated by multiplying fractional cloud sky cover times cloud thickness times oceanic and continental area. Low cloud cover over the ocean was taken to be 50% [Warren et al., 1988] with a cloud thickness defined to be 500 m [Warneck, 1999]. Low cloud cover over the continents was taken to be 30% [Warren et al., 1986] with a cloud thickness defined to be 1000 m [Warneck, 1999]. Only low clouds with liquid water have been considered. The tropospheric cloud volume estimated here is similar to the Liang and Jacob [1997] estimate of 10%, which compared well with satellite derived column liquid water contents. The resulting global aqueous loss estimate for methanol via HO reaction in cloud is 10 Tg methanol yr−1 and listed in Table 4. A loss of 10 Tg methanol yr−1 represents an additional loss equal to 25% of the total loss estimated by Singh et al. [2000] but is less than 5% of the total loss estimated here. The relative uncertainties in global cloud volume, water content, aqueous [HO], aqueous [CH3OH], and rate constant are estimated at 30% for each and results in approximately a factor of 2 uncertainty in the aqueous HO-methanol chemical sink.

Table 2b. Representative Atmospheric Methanol Concentrations, ppt or μM
 Typical ValueRangeDetails
Boundary Layer, ppt
Arctic winter/spring25030–600 
Arctic summer800400–1200 
Background Ocean900300–1400 
Background Continent20001000–4000 
Grassland60004000–9000 
Forest100001000–37000 
Urban2000030–47000 
 
Aloft, ppt
Free Troposphere600300–1200 
 
Rain Estimated Range, micro-Molar (μM)
Rain Equilibrium Estimates for Temperatures of:0 deg-C25 deg-CH; Snider and Dawson [1985]
  Background Ocean0.90.2CH3OH = 900 ppt
  Urban204CH3OH = 20000 ppt

[9] Methanol loss on aerosols is not considered here. Iraci et al. [2002] examined methanol uptake by sulfuric acid aerosols and, while the solubility of methanol is dramatically enhanced at the sulfuric acid concentrations (40–75% by weight) and temperatures (197–241°K) considered and aqueous rates of reaction in these aerosols are also enhanced, they concluded sulfuric acid aerosols have a negligible impact on atmospheric aerosol because of the small aerosol liquid volume involved. We believe this will be the case for other aerosol compositions.

2.2. Ocean and Land Precipitation Deposition

[10] “Wet” deposition losses are estimated to be 10 Tg methanol yr−1 and this is also equal to 25% of the total estimated by Singh et al. [2000] and <5% of the methanol loss estimated here. Wet deposition was calculated by assuming thermodynamic equilibrium between the gas phase and precipitation water. Snider and Dawson [1985] have reported the sole measurement of methanol in precipitation. Their atmospheric gas phase measurement of 2600 pptv, rain measurement of 690 nM, and Henry's Law measurements show the system was near thermodynamic equilibrium. This suggests the equilibrium assumption to be a reasonable approximation. Precipitation rates for land and ocean were taken from work by Peixoto and Oort [1992] and convolved with the background oceanic and continental values of Table 2b to estimate the wet deposition to land, 5 Tg methanol yr−1, and to the ocean, 5 Tg methanol yr−1. These are listed in Table 4. The range is evaluated from variances in concentration, Henry's Law constant (temperature) and precipitation estimates.

2.3. Gas Phase HO Reaction

[11] A similar calculation was performed to estimate the gas phase loss of methanol by reaction with HO. A three-box model of the atmosphere was applied. The lowest 2 km of the troposphere was considered in two parts, one oceanic with a methanol concentration of 900 pptv and the other continental with a concentration of 2000 pptv. A third box represented the global free troposphere with a methanol concentration of 600 pptv. HO was assumed constant for all three boxes at a concentration of 1 × 106 molecules cm−3 in keeping with the global mean annual tropospheric estimate of Prinn et al. [1995]. The gas phase methanol-HO reaction rate constant was taken to be 8 × 10−13 cm3 molecule−1 s−1. The resulting gas phase photochemical loss of methanol is 100 Tg methanol yr−1, about 37% of its loss, and listed in Table 4. This value is about 2.5 times that estimated by Singh et al. [2000] for the same process. It is nearly identical to those estimated using global HO fields from the model of Bey et al. [2001] for January, 101 Tg methanol yr−1, and July, 105 Tg methanol yr−1. We have adopted a loss rate of 100 Tg methanol yr−1 and acknowledge that the variability in methanol HO loss is large.

2.4. Ocean and Land “Dry” Deposition

[12] Surface deposition can occur through “dry” and “wet” processes to land and ocean. A typical means of estimating the air-to-surface flux is through the concept of the deposition velocity, Vs, [e.g., Wesely and Hicks, 2000] which assumes the flux is proportional to the bulk air-surface concentration gradient and a transfer coefficient with units of velocity. Singh et al. [2000] assumed a Vs of 0.1 cm s−1 to estimate methanol deposition loss to land and ocean surfaces. We have reevaluated the surface dry depositional loss of methanol to the ocean and to land using the Wesely [1989] resistance model to estimate Vs for various land types and seasons and for the Vs to the ocean [Duce et al., 1991]. In this scheme aerodynamic, chemical-physical properties, material surface, and chemical reactivity considerations are treated as a series of resistances. For methanol, an oceanic Vs of 0.4 cm s−1 is expected at a wind speed of 5 m s−1 and Vs would increase to 1.1 cm s−1 for 10 m s−1 winds. On land, peak Vs is 0.9 cm s−1 for summer forest conditions under full sun and 0.04 at night. Vs's estimated for other vegetation types, times of day, and seasons lie within these values. Wesely and Hicks [2000] have reviewed measured Vs's for low molecular weight organic peroxides and organic acids and report Vs's of 0.5–1.1 cm s−1 for formic acid. Organic peroxide surface resistances of 0.1–15 s cm−1 were listed implying Vs's of ∼0.06–10 cm s−1. A value of 10 cm s−1 is extreme. Methanol should behave similarly to organic peroxides based upon physical properties and biological reactivity. The continental Vs is set to 0.4 cm s−1. The “typical” atmospheric surface concentrations from Table 2b were combined with the Vs estimates to calculate the “dry” deposition loss of methanol to land and ocean and these are listed in Table 4. Ranges were estimated by assigning a factor of 2 uncertainty on Vs and noted ranges in concentration. The global total “dry” depositional loss is estimated at 150 Tg methanol yr−1.

2.5. Total Loss Estimate

[13] The total global annual loss of methanol from the atmosphere is 270 Tg methanol. This is approximately a factor of 5 larger than that estimated earlier. It is also about 2–3 times the earlier source estimate. The lower range loss estimate is also 50% in excess of the earlier source value. Hence, our analysis of losses shifts the methanol budget from being a factor of 2 heavy in sources to being a factor of 2 heavy in sinks.

3. Methanol Sources Reconsidered

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[14] The magnitude of the above total estimated methanol sink necessitated a reconsideration of global methanol sources. Emissions from fossil fuel combustion, biomass burning, and plant decay vary slightly from those estimated by Singh et al. [2000]. We have estimated fossil fuel emissions based upon the relationship between methanol and total reactive odd nitrogen (NOy) noted by Goldan et al. [1995a]. The emissions from biomass burning were estimated using the average methanol-CO (carbon monoxide) ratio reported by Yokelson et al. [1999] and Goode et al. [2000] from their reviews of the literature. Fossil fuel nitrogen oxide emissions and biomass burning CO were taken from their respective global budget estimates in Brasseur et al. [1999]. The methanol source from plant matter decay is taken from Warneke et al. [1999]. The model of Bey et al. [2001] was used to evaluate photochemical methanol production in the atmosphere. Methanol source rates from these four processes are listed in Table 4. The range estimates are from propagating stated parameter variances. Methanol emissions from primary biogenic and oceanic sources exhibit the greatest uncertainty and are considered separately below.

3.1. Primary Biogenic Source Uncertainty

[15] Guenther et al. [1995] formulated a global emission inventory of biogenic volatile organic carbon, VOC, and as a part of that effort assigned a single emission factor to be applied to a VOC category that included methanol and a variety of other VOCs with poorly understood emission processes. The total global emission of this other VOC category was estimated to be 260 Tg carbon yr−1. In that analysis, using very limited information from laboratory measurements of methanol emission from leaves [e.g., MacDonald and Fall, 1993], the primary biogenic source of methanol, was suggested to be in the range of >100 Tg carbon yr−1 (a value of 280 Tg methanol yr−1 is used here). Since the Guenther et al. [1995] model calculates a global emission of 260 Tg carbon yr−1 for methanol and other VOC using an emission factor of 1.5 μg C g−1 h−1, a global methanol emission of 100 Tg carbon yr−1 would require an average methanol emission factor of 0.57 μg C g−1 h−1, which represents >0.2% of global terrestrial primary production.

[16] Subsequently, several investigators have measured methanol emissions from vegetation in both laboratory and field settings, and this data is summarized in Table 3. Several brief generalizations can be made from laboratory investigations: (1) young, rapidly dividing leaves show the greatest emission rate; (2) emissions in undisturbed leaves are highest when transpiration is highest; (3) methanol emissions from conifers are lower than from broad-leaf plants; and (4) methanol releases are greatly enhanced by leaf wounding [MacDonald and Fall, 1993; Nemecek-Marshall et al., 1995]. Mean methanol fluxes ranging from 0.5–31 μg C g−1 h−1 were obtained with a variety of plants. Most of these values are much higher than the conservative value of 1.5 μg C g−1 h−1 used by Guenther et al. [1995] for methanol plus other VOC. However, Holzinger et al. [2000] have reported a laboratory study with Mediterranean holm oak, which shows a much lower flux of about 0.5 μg C g−1 h−1, illustrating the need for further careful measurements of methanol emission factors in a variety of plants. These results also point out the difficulty in assigning a global methanol emission factor, since leaf emissions are so dependent on leaf age and stomatal transpiration, factors that vary considerably during the growing season.

Table 3. Measurements of Methanol Emissions From Vegetation
SourceMethanol FluxReference
RangeMean
Laboratory
Diverse species (14)0.2–18.4 μg C g−1 h−15.4 μg C g−1 h−1MacDonald and Fall [1993]
Bean and cottonwood leaves5–65 μg g−1 h−1 (bush bean); 5–50 μg g−1 h−1 (soybean); 1–70 μg g−1 h−1 (cottonwood)≈7.5 μg C g−1 h−1Nemecek-Marshall et al. [1995]
Aspen leaves (young)75–114 μg g−1 h−131 μg C g−1 h−1R. Fall (unpublished)
Mediterranean holm oak (leaf dry wt.); minimum root flooded, maximum young leaf0.08–1.4 μg C g−1 h−10.5 μg C g−1 h−1Holzinger et al. [2000]
 
Field
Grass0.9–1.3 mg m−2 h−1 Kirstine et al. [1998]
Clover9–20 mg m−2 h−1  
Grassland 0.46 ± 0.07 mg m−2 h−1 (noon, 2 yr average; 1.4 ± 0.2 μg g−1 h−1)Fukui and Doskey [1998]
Sub-alpine conifer forest ≈1 mg m−2 h−1Baker et al. [2001]
Pine forest ≈4 mg m−2 h−1 (daily maximum, 2 mo average)Schade and Goldstein [2001]
Hayfield1–8.4 mg m−2 h−1 Karl et al. [2001]
Alfalfa fieldUndisturbed: 12.9 mg m−2 24 h−1 After cutting (3 different days): 25.5–35.2 mg m−2 24 h−1≈1 mg m−2 h−1 (24 h average)Warneke et al. [2002]
Rain forest1–5 μg C g−1 h−1 (various leaves)≈1.3 mg m−2 h−1Geron et al. [2002]

[17] A variety of field measurements generally support the assumptions used by Guenther et al. [1995] to derive their methanol emission estimate, and this information is also shown in Table 3. For example, Kirstine et al. [1998] and Fukui and Doskey [1998] examined VOC release in grasses or grassland and found methanol emission rates in the range of 0.5 to 20 mg m−2 h−1, with higher emissions in disturbed vegetation, consistent with laboratory findings that methanol pools exist in leaves and are released upon wounding. A variety of other field measurements [Baker et al., 2001; Schade and Goldstein, 2001; Karl et al., 2001; Warneke et al., 2002; Geron et al., 2002] in many different ecosystems give methanol fluxes (growing season) in the range of 0.5–4 mg m−2 h−1 (Table 3). When expressed on a leaf dry weight basis these values generally argue for a methanol emission factor higher than that estimated by Guenther et al. [1995]. It is noteworthy that the Guenther et al. [1995] emission factor for VOC is dependent only on temperature. If we estimate global methanol emissions using the algorithm that Guenther et al. [1995] used for isoprene, which assumes that emissions are reduced in the dark, and assume that methanol emissions are greatly reduced for older leaves, then we would need a methanol emission factor, for young leaves exposed to sunlight, of about 4 μg C g−1 h−1 in order to get the same global emission rate. However, given the lack of methanol flux measurements in different ecosystems over the growing season, retaining the conservative emission factor seems justified.

[18] The above consideration of loss processes, totaling 270 Tg methanol yr−1 also argues for a larger vegetative methanol source closer to that given by Guenther et al. [1995]. In Table 4, the primary biogenic source minimum and maximum are those of Singh et al. [2000] and Guenther et al. [1995], respectively. This source is for terrestrial vegetation emissions alone.

Table 4. Estimated Methanol Global Inventory, Tg-methanol, and Its Sources and Sinks, Tg-methanol yr−1
DescriptionValueRangeComment
Methanol Mass, Tg
   Free troposphere2.52.5600 pptv
   Marine BL0.70.5–0.9Zbl = 1km; 900(600–1200) pptv
   Continental BL0.70.5–3.5Zbl = 2km; 2000(1500–4000) pptv
Total mass3.93.5–6.9 
 
Sources, Tg-methanol yr−1
   Primary anthropogenic85–110.17*NOx emissions; after Goldan et al. [1995a] and fossil fuel NOx from Brasseur et al. [1999]
   Primary biogenic28050–>280poorly constrained (e.g., >280 Tg-methanol yr−1 [Guenther et al. [1995, 1999]; 50–125 Singh et al. [2000]
   Methane oxidation3018–3018 from Singh et al. [2000] and 30 from Bey et al. [2001] 3-D models, respectively.
   Plant matter decay2010–4018–40 Warneke et al. [1999]; 10–40 Singh et al. [2000]
   Biomass burning122–321.6 (0.6–3.1)% of CO biomass burning emission, Yokelson et al. [1999]; Goode et al. [2000]; Brasseur et al. [1999]
   Ocean???0–8030 Tg-methanol yr-1, assumes oceanic emissions compensate for oceanic dry deposition minus FT-MBL exchange.
Source total34590–490 
 
Sinks, Tg-methanol yr−1
   Dry deposition land7035–210Vs = estimated from CH3OOH [Wesely, 1989], MeOH= 2000 pptv continental background, 10000 pptv grassland/forest; 65 Tg-methanol yr−1 spring + summer; 5 Tg-methanol yr−1 fall + winter
   Dry deposition ocean8060–150Vs = 0.42 cm/s for wind = 5m/s, (1.1 at 10 m/s; est. Duce et al. [1991]), MeOH = 900 pptv oceanic to 2000 continental background
   Wet deposition ocean51–16equilibrum; H(MeOH) from Snider and Dawson [1985], MeOH = 900 pptv, precipitation Peixoto and Oort [1992]
   Wet deposition land53–20equilibrium; H from Snider and Dawson [1985], MeOH = 2000 pptv, precipitation Peixoto and Oort [1992]
   Aqueous HO reaction105–20lwc = 3e-7 L/L; HO = 0.2(0.1–0.4)e-12 M; k = 1e9; MeOH = 900 (2000) pptv; H(MeOH) = 1000 M/atm; 50(30)% cloud cover; 0.5(1)km cloud thickness
   Gaseous HO reaction10025–1503D model [HO] of Bey et al. [2001]: assumed methanol of FT = 600 pptv, CBL = 2000 pptv, MBL = 900 pptv
Sink total270160–570 
 
Methanol Lifetimes, Days
   Gas reaction 18τOH based on work by Bey et al. [2001]
   Cloud reaction 111τcloud = 1/(k[HO])/fc/ft/fd; k = 1e9 1/M/s; [HO] = 0.2e-12 M; fc = HRTL/(1 + HRTL); H = 1000, RT = 22.4, L = 3e-7; ft = cloud time fraction 15(10–20)%; fd = fraction of day light 50%;
   Surface deposition 24Zbl/Vs/fbl; cont. (Vs = 0.4 cm/s; Zbl = 2km); ocean (Vs = 0.4 cm/s; Zbl = 1km); fbl = fraction of time in BL 15(10–20)%
Composite Lifetime 9gas HO, cloud HO, precipitation, surface deposition

3.2. Ocean Source

[19] Methanol input to the atmosphere would be higher with the inclusion of a hypothesized but unquantified oceanic source [Singh et al., 2000]. An oceanic source of methanol is inferred from photochemical modeling studies of the remote MBL [Chang, 2002] and discussed in section 3.2.1. The ocean source needed to satisfy the model and atmospheric observations is estimated at 30 Tg methanol yr−1 with a range estimate of 0–80 Tg methanol yr−1. The limits are heuristic. The lower value stems from an assumption that methanol is readily dissolved in seawater and consumed rapidly by bacteria and other organisms. The upper limit derives from the maximum flux needed to maintain observed MBL methanol mixing ratios over the subtropical remote ocean for a case without FT-MBL material exchange.

[20] The likelihood of a global oceanic methanol source equal to 30 Tg methanol yr−1 is difficult to evaluate. Observations of methanol in seawater have not been reported. In situ oceanic methanol sources are speculative, principally biological, and expected to be temporally and spatially inhomogeneous. Sieburth [1988] and Sieburth and Keller [1989] indicated that bacterial consortia are able to transform algal carbohydrates to methanol within the aerobic upper ocean. Further support of oceanic biological methanol formation comes from D. Riemer (unpublished data, 1998), who observed methanol in the headspace gas of laboratory phytoplankton cultures (Table 5); an example of culture data is shown in Figure 1. Assuming a Henry's Law constant of 200 M atm−1 (appropriate to fresh water at T = 25°C), the observed methanol mixing ratios suggest culture seawater methanol concentrations >1 × 10−6 M. This concentration is close to that reported by King et al. [1983] for in situ sediment water from a Maine tidal anoxic sediment, 2 × 10−6 M. While Riemer's experiments were focused upon the determination of isoprene production [Milne et al., 1995], the methanol observations imply its production within the cultures. Methanol was observed with all cultures during exponential and stationary phase growth. Since marine phytoplankton are the most abundant organisms on Earth and their primary production is equal to terrestrial primary production, even production of small amounts of methanol would be a very significant global source.

image

Figure 1. Headspace methanol and isoprene and cell count during laboratory culture experiment with Amphidinium aperculatum.

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Table 5. Monoalgal Culture Studies of Methanol Producers (After Milne et al. [1995])a
OrganismMethanolbIsoprenec
Diatoms
Biddulphia mobiliensis++
Phaeodactylum tricornutum++
Thalassiosira weissflogil++
Chaetoceros affinis++
Skeletonema costatum++
 
Coccolithophores
Emiliania huxleyi++
 
Dinoflagellates
Amphidinium aperculatum++
Heterocapsa pygmaea++
 
Others
Prymnesium parvum++
Synechococcus sp++

[21] Oceanic methanol sink processes should also be considered in an assessment of ocean methanol. Briefly, these include photochemical loss and microbial uptake. Again studies of methanol consumption in seawater have not been reported. Methanol does not readily photolyze in air or seawater. It is relatively unreactive with hydrated electrons, superoxide or perhydroxyl. It does react with HO in water and a simple methanol HO-lifetime estimate is ≥40 days, where τHO = 1/k/[HO]sw, the seawater [HO]sw concentration is <3 × 10−16 M [Mopper and Zhou, 1990], and k = 1 × 109 M−1 s−1 as above. Thus, methanol is long-lived with respect to photochemical oxidation. Kiene [1993] suggested methanol as a carbon and energy source for oceanic methylotrophic organisms (these bacteria are often cultured in a medium containing methanol) and stated little was known about methanol's biogeochemical cycling. A rate for oceanic bacterial methanol uptake is not known but we estimate it has a 3-day lifetime based on experimental biological turnover times for DMSP (dimethylsulfoniopropionate) [Simo et al., 2000], methylamines [Yang et al., 1994], and formaldehyde [Mopper and Kieber, 1991], and inferred GBT (glycine betaine) turnover times [Kiene and Hoffmann-Williams, 1998; Gibb et al., 1999].

[22] For comparison, atmospheric acetone, like methanol, also has an implied ocean emission. Jacob et al. [2002] inferred an oceanic source of acetone of 17 Tg carbon yr−1 using a global photochemical inverse model calculation. The model included acetone deposition to the oceans and a net flux out of the ocean was predicted. On a grams of carbon basis, our inferred methanol oceanic source is approximately two thirds of their acetone source, but our calculations (Table 4) suggest the ocean is a net methanol sink.

[23] Several possible methanol formation schemes are briefly outlined below involving biological processes or chemistry. The emphasis is placed on identifying which of these speculative processes are capable of methanol production at the rate implied by the MBL modeling study.

3.2.1. Air-To-Sea Transport

[24] Atmospheric measurements of methanol in the remote marine boundary layer (MBL) show concentrations of about 900 pptv on average with slightly lower concentrations, approximately 600 pptv, in the free troposphere (FT) [Singh et al., 2000, 2001]. A one-dimensional model of MBL methanol photochemistry with seawater methanol concentrations set to 0 showed methanol to deplete in the tropical-subtropical MBL with about a 3-day lifetime due to surface deposition [Chang, 2002]. It was not possible for this model to predict observed remote MBL methanol levels. Inclusion of photochemical methanol production alone led to predicted mixing ratios <120 pptv. The addition of FT-to-MBL transport raised the calculated methanol mixing ratio to 450 pptv and 700 pptv when FT mixing ratios were assumed to be 900 and 1800 pptv, respectively. The latter is a high estimate from Singh et al. [2001]. Oceanic methanol emissions were required for the model to sustain methanol mixing ratios at the observed MBL level (900 pptv). In the case of photochemistry alone, gross oceanic emissions were required to be nearly equal to the gross rate of surface depositional loss, thereby, reducing the net methanol flux to near zero. For this case, a net zero flux implied an oceanic source of 80 Tg yr−1 and implied an oceanic surface film concentration between 0.2 and 2.0 × 10−6 M depending upon temperature. This is the maximum emission listed in Table 4. In the case where FT to MBL exchange is included, gross oceanic emission rates of 1/4 to 1/2 those of the gross surface deposition, 20–40 Tg methanol yr−1, were required and this implies a surface concentration of 0.05–0.5 × 10−6 M. This case was used to define the nominal ocean emission rate of 30 Tg methanol yr−1 and serves as the target value for the oceanic sources described below.

3.2.2. Methyl Halide Hydrolysis

[25] Zafiriou [1975] and Elliot and Rowland [1995] proposed that methanol could be produced by the hydrolysis of methyl halides emitted by phytoplankton. The global methanol production rate from methyl halides hydrolysis is quite small and totals less than 0.3 Tg methanol yr−1 based on the work of Moore et al. [1996] for methyl chloride, Anbar et al. [1996] for methyl bromide, and Moore and Groszko [1999] for methyl iodide. This process is unimportant to atmospheric methanol.

3.2.3. Methane Oxidation

[26] Fugitive emissions from methanogenic and methanotrophic organisms in the upper water column [e.g., Sieburth et al., 1987; Sieburth and Keller, 1989; Kiene, 1993], could result in seawater methanol due to inefficiencies in the methane-methanol-formaldehyde-formate biochemical coupling. However, such inefficiencies are unlikely given the fact methanol is a key intermediate in yielding energy from methane oxidation. Regardless, an upper limit for this source can be estimated for the upper ocean (Our focus is on atmospheric methanol and we have restricted the discussion to the upper ocean and have ignored methane oxidation at depth where sediment emissions from methanogens or hydrate dissociation can be significant and methane oxidation rates high). Cicerone and Oremland [1988] and Holmes et al. [2000] have estimated upper ocean methane production at 5–20 Tg carbon yr−1. Holmes et al. [2000] estimated that less than 2% of the methane produced in the upper oligotrophic North Atlantic and North Pacific is oxidized there. While the fraction of methane oxidized in the upper ocean appears to increase with increasing nutrients toward the coast and in estuaries [e.g., Ward et al., 1987, 1989; Jones, 1991; Bange et al., 1994; Tsurushima et al., 1996; Sansone et al., 1998; Holmes et al., 2000; Jayakumar et al., 2001] and methane oxidation turnover time decreases sharply with methane concentration above 15 nM to lifetimes <5 yr [e.g., Valentine et al., 2001], nearly all upper ocean methane appears to be simply lost to the atmosphere. If the ∼2% of the oxidized methane [Holmes et al., 2000] went directly to methanol and all of this went into the atmosphere, the maximum oceanic methane-to-methanol production rate would be <0.53 Tg methanol yr−1. This is a vanishingly small source of atmospheric methanol.

3.2.4. Methylation/Demethylation Biochemical Cycles

[27] The presence of carboxymethyl groups is well documented in the proteins and polysaccharides of living organisms. The hydrolysis of these methyl esters by acid- or base-catalyzed reactions, or by methylesterase enzymes results in the formation of methanol.

[28] For example, the methanol source in vegetation (section 3.1) is thought to be primarily plant cell wall pectin, a polysaccharide rich in methyl ester linkages, that are enzymatically hydrolyzed, releasing methanol during cell wall expansion [Fall and Benson, 1996]. In marine systems, however, pectin is not common in the cell walls of phytoplankton and seaweeds, which contain other types of polysaccharides, such as alginates, mannans, xylans, and sulfated polysaccharides, in addition to cellulose (www.biologie.uni-hamburg.de/b-online/e26/26d.htm). Only the sulfated polysaccharides contain significant amounts of methyl groups, where the methyl groups are linked by very stable ether linkages. It is notable that this type of methylated polysaccharide is reported to occur in most marine algae [Painter, 1983]. If the turnover of such residues in the food chain results in demethylation to form methanol, as in lignin degradation by fungi [Fall and Benson, 1996], this might be a potentially large source of marine methanol, given the abundance of marine phytoplankton and their consumption in the food web.

[29] It is tempting to think that some fraction of the abundant methylated osmoprotectants in marine organisms might be a methanol source. These protectants are characterized as highly methylated quaternary amino or tertiary sulfonium groups. For example, the annual turnover of the osmolyte, DMSP, in phytoplankton gives rise to oceanic emissions of 15–33 Tg S as CH3SCH3 [Simo et al., 2000]. In addition, Visscher and Taylor [1994], Simo et al. [2000], and Kiene et al. [2000] have described bacteria utilizing DMSP as a source of carbon and energy. Although these types of bacteria are generally methanol consumers (methylotrophs), Kiene et al. [2000] estimated ocean DMSP utilization yields 3–90 × 10−9 M d−1 of unspecified methylated compounds and CO2. Assuming (1) 1% of the total methylated material is released as methanol, (2) it is produced uniformly in the top 10 m of the ocean, and (3) it is delivered to the atmosphere then, the global methanol production rate would be 2–54 Tg yr−1. Simo et al. [2000] observed a 3-day turnover time for DMSP and a similar methanol production estimate of 2–20 Tg yr−1 is calculated using their turnover time and assuming surface DMSP concentrations of 10−8–10−7 M, a 10 m thickness, and 1% methanol yield. DMSP consumption by bacteria is of the right order of magnitude to that needed. Compensating variations in DMSP concentration, yield, and surface ocean thickness would maintain this rate. For example, increasing the yield to 10% and decreasing the thickness to 1 m gives the same rate of methanol production.

[30] Similar speculative estimates of the fate of another important marine osmolyte, GBT, might also support a significant methanol source. As with DMSP, GBT-degrading bacteria are able to demethylate GBT [Sieburth and Keller, 1989]. Seawater GBT concentrations are unknown but estimated to be on the order of 1–10 × 10−9 M [Kiene et al., 1998; Kiene and Hoffmann-Williams, 1998]. Kiene and Hoffmann-Williams [1998] studied GBT biodegradation, and could account for only 41–91% of the GBT in their degradation experiments, and suggested the missing fraction went into soluble and volatile products. Kiene et al. [1998] argued that the biogeochemical cycling and turnover of GBT would be comparable to the turnover of DMSP. It remains to be determined if methanol is a product of GBT turnover. Other marine sources of methanol, could include methanol arising from protein repair pathways [Kagan et al., 1997] or as a result of protein demethylation during chemotaxis [Grebe and Strock, 1998], but the magnitude of such methanol production is uncertain. Finally, it should be noted that little is known of the metabolites arising from other levels of the marine food web. As a large amount of carbon is processed annually in this food web, it is probable that unknown marine methanol sources exist.

3.2.5. Other Marine C1 Observations

[31] Formaldehyde and formate are subject to photochemical and biological formation and loss and have been measured in seawater. Formaldehyde ranges from 4–16 × 10−9 M for the open ocean and 10–40 × 10−9 M for coastal waters [Mopper and Stahovec, 1986; Kieber and Mopper, 1990; and Zhou and Mopper, 1997]. Surface microlayer concentrations in these systems are approximately a factor of 10 higher, ranging from 35 × 10−9 M to 45–170 × 10−9 M, respectively [Zhou and Mopper, 1997]. Zhou and Mopper also determined formaldehyde in air near the ocean surface and concluded the ocean-atmosphere were near equilibrium such that at specific times and locations the ocean could be a source of formaldehyde, a compound with an effective solubility constant 10 times that of methanol. One of the arguments expressed against the idea of an oceanic source of methanol is its “large” solubility in water, an argument which would not hold up in the case of formaldehyde. Formate concentrations are 80–190 × 10−9 M, 200–800 × 10−9 M, and 100–250 × 10−9 M, respectively, from the Sargasso Sea, Biscayne Bay, and Orinoco estuarine water [Kieber et al., 1988; Vaughan and Mopper, 1990]. Should methanol concentrations prove similar to formaldehyde in the surface microlayer or to formate, they would be on the order of 50 × 10−9 M. This concentration is approximately that required to support the methanol oceanic gross emission rate above.

4. Terrestrial Net Fluxes

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[32] Methanol fluxes have been measured above some terrestrial plant canopies including conifer forests [Schade and Goldstein, 2001; Baker et al., 2001], tropical rain forest [Geron et al., 2002], harvested hayfields [Karl et al., 2001] and an alfalfa field before and after harvesting [Rinne et al., 2001; Warneke et al., 2002]. These investigators measured net methanol fluxes using either the relaxed eddy accumulation technique or eddy covariance methods [e.g., Wesely and Hicks, 2000]. The reported net methanol fluxes can be used to evaluate the terrestrial methanol source and sink estimates described above. The total terrestrial biogenic source (live vegetation plus plant matter decay) of 300 Tg methanol yr−1 (see Table 4) can be distributed among individual ecosystem types using the model of Guenther et al. [1995]. This procedure predicts annual total methanol emissions of 0.44 g m−2 for subalpine conifer forests, 0.55 g m−2 for cool temperate conifer forests, 0.74 g m−2 for irrigated croplands, and 3.9 g m−2 for tropical rain forests. Schade and Goldstein [2001] observed average daily net methanol fluxes of about 15 mg C m−2 from July to mid September from a cool temperate conifer forest. The total flux of about 1 g m−2 observed for the duration of their study is probably considerably less than the annual total since similar or higher fluxes are expected for at least May and June at this site. The predicted contribution of this landscape to the global annual emission (0.55 g m−2) is lower than the observed net flux. The other studies report fewer observations and are more difficult to extrapolate but the results suggest daily methanol fluxes of about 8 to 13 mg C m−2 and annual fluxes of about 0.6 g m−2 for subalpine conifer forest, 1 g m−2 for irrigated crops and 3 g m−2 for tropical rain forests. In each case, the net flux estimates based on field measurements are similar to the predictions associated with the global source estimate. Since the observed net flux should be considerably less than the predicted emission at these sites, due to the expected deposition rates, this evaluation demonstrates our limited understanding of the methanol budget for terrestrial landscapes. However, these results argue for a terrestrial ecosystem source that is at the high end of previous estimates.

5. Summary

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[33] The mass of methanol in the atmospheric reservoir, the mass rate of methanol sources and sinks, and the estimated atmospheric lifetime of methanol in the free troposphere, MBL, CBL, and in-cloud, are summarized in Table 4. The methanol source and sink total 340 and 270 Tg methanol yr−1, respectively. The uncertainty in either value remains large, ±200 Tg methanol yr−1. The sink value derived here is approximately 6 times that estimated by Singh et al. [2000] and it is about 3 times their estimated source. This sink value is much closer to a total source calculated using Guenther et al.'s biogenic emissions, >280 Tg methanol yr−1, and this source value was adopted. It is important to note that sources still exceed sinks, here by about 25%, and this will be made larger with the inclusion of an oceanic methanol source. The greatest uncertainties can be found in the estimates of biogenic emissions and dry deposition suggesting continued methanol study is required in this area. Losses of methanol by precipitation and by in-cloud aqueous reaction are noted. These are thought to be small in this analysis but comprise a significant sink when compared with prior total sink estimates. In the case of clouds and seawater, analytical methods are unreported and observations are unavailable with which to begin to critically assess methanol concentrations in these media and assess their significance in methanol loss. Additional rain and snow methanol measurements are needed to refine precipitation removal estimates.

[34] The implied flux of methanol from the atmosphere to the ocean and its biogeochemical cycling in the surface ocean is intriguing. The amount of methanol introduced from the air exceeds the amount of methane produced in the open ocean column. Add to this methanol, the methanol production argued for in the upper ocean, then these ubiquitous sources could be sustaining methylotrophic organisms throughout the surface ocean.

Acknowledgments

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

[35] D.J.J. and B.D.F. were partially supported by the National Science Foundation-Atmospheric Chemistry. B.G.H. and D.D.R. were partially supported by the National Aeronautics and Space Administration-Global Tropospheric Experiment. R.F. acknowledges support by NSF grant ATM-9805191. H.B.S. would like to thank the NASA Interdisciplinary Science Program and Tropospheric Chemistry Program for support. We thank Ronald Kiene for sharing his insights on methyl-group oxidation and Jan Bottenheim, Hacene Boudries and their colleagues for providing a preprint including their ALERT2000 methanol observations, and Thomas Karl, Chris Geron and Joost de Gouw for sharing unpublished data.

References

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information
  • Anbar, A. D., Y. L. Yung, and F. R. Chavez, Methyl bromide: Ocean sources, ocean sinks, and climate sensitivity, Global Biogeochem. Cycles, 10, 175190, 1996.
  • Anderegg, R. J., R. Betz, S. A. Carr, J. W. Crabb, and W. Duntze, Structure and function of Saccharomyces cerevisiae mating hormone a-factor, J. Biol. Chem., 263, 18,23618,240, 1988.
  • Baker, B., A. Guenther, J. Greenberg, and R. Fall, Canopy level fluxes of 2-methyl-3-buten-2-ol, acetone, and methanol by a portable relaxed eddy accumulation system, Environ. Sci. Technol., 35, 17011708, 2001.
  • Bange, H. W., U. H. Bartell, S. Rapsomanikis, and M. O. Andreae, Methane in the Baltic and North Seas and a reassessment of the marine emissions of methane, Global Biogeochem. Cycles, 8, 465480, 1994.
  • Bey, I., D. J. Jacob, R. M. Yantosca, J. A. Logan, B. D. Field, A. M. Fiore, Q. B. Li, H. G. Y. Liu, L. J. Mickley, and M. G. Schultz, Global modeling of tropospheric chemistry with assimilated meteorology: Model description and evaluation, J. Geophys. Res., 106, 23,07323,095, 2001.
  • Boudries, H., J. W. Bottenheim, C. Guimbaud, A. M. Grannas, P. B. Shepson, S. Houdier, S. Perrier, and F. Dominé, Distribution and trends of oxygenated hydrocarbons in the high Arctic derived from measurements in the atmospheric boundary layer and interstitial snow air during the ALERT2000 field campaign, Atmos. Environ., Special Issue ALERT2000 and SUMMIT2000, in press, 2002.
  • Bouhamra, W. S., Indoor air quality in Kuwaiti house: Pollutants and their concentrations, Kuwait J. Sci. Eng., 23, 209215, 1996.
  • Brasseur, G. P., J. J. Orlando, and G. S. Tyndall (Eds.), Atmospheric Chemistry and Global Change, Oxford Univ. Press, New York, 1999.
  • Cavanagh, L. A., C. F. Schadt, and E. Robinson, Atmospheric hydrocarbon and carbon monoxide measurements at Point Barrow, Alaska, Environ Sci. Technol., 3, 251257, 1969.
  • Chang, W., Influence of turbulent transport and chemistry on the distributions of H2O2, CH3OOH, and CH2O in the remote marine boundary layer, Ph.D. thesis, Univ. of R. I., Kingston, R. I., 2002.
  • Cicerone, R. J., and R. S. Oremland, Biogeochemical aspects of atmospheric methane, Global Biogeochem. Cycles, 2, 199327, 1988.
  • de Paula Pereira, P. A., E. T. Sousa Santos, T. de Freitas Ferreira, and J. B. de Andrade, Determination of methanol and ethanol by gas chromatography following air sampling onto florisil cartridges and their concentrations at urban sites in the three largest cities in Brazil, Talanta, 49, 245252, 1999.
  • Doskey, P. V., and W. Gao, Vertical mixing and chemistry of isoprene in the atmospheric boundary layer: Aircraft-based measurements and numerical modeling, J. Geophys. Res., 104, 21,26321,274, 1999.
  • Duce, R. A., et al., The atmospheric input of trace species to the world ocean, Global Biogeochem. Cycles, 5, 193259, 1991.
  • Elliott, S., and F. S. Rowland, Methyl halide hydrolysis in natural waters, J. Atmos. Chem., 20, 229236, 1995.
  • Fall, R., Cycling of methanol between plants, methylotrophs and the atmosphere, in Microbial Growth on C1 Compounds, edited by M. Lidstrom, and R. Tabita, pp. 343350, Kluwer Acad., Norwell, Mass., 1996.
  • Fall, R., Biogenic emissions of volatile organic compounds from higher plants, in Reactive Hydrocarbons in the Atmosphere, edited by C. N. Hewitt, pp. 4196, Academic, San Diego, Calif., 1999.
  • Fall, R., and A. A. Benson, Leaf methanol-the simplest natural product from plants, Trends Plant Sci., 1, 296301, 1996.
  • Fehsenfeld, F., et al., Emissions of volatile organic compounds from vegetation and the implications for atmospheric chemistry, Global Biogeochem. Cycles, 6, 389430, 1992.
  • Fukui, Y., and P. V. Doskey, Air-surface exchange of nonmethane organic compounds at a grassland site: Seasonal variations and stressed emissions, J. Geophys. Res., 103, 13,15313,168, 1998.
  • Geron, C., A. Guenther, J. Greenberg, H. Loescher, D. Clark, and B. Baker, Biogenic volatile organic compound emissions from a rain forest in Costa Rica, Atmos. Environ., 36, 37933802, 2002.
  • Gibb, S. W., R. Fauzi, C. Mantoura, P. S. Liss, and R. G. Barlow, Distributions and biogeochemistries of methylamines and ammonium in the Arabian Sea, Deep Sea Res., Part II, 46, 593615, 1999.
  • Goldan, P. D., et al., Measurements of hydrocarbons, oxygenated hydrocarbons, carbon monoxide, and nitrogen oxides in an urban basin in Colorado: Implications for emission inventories, J. Geophys. Res., 100, 22,77122,783, 1995a.
  • Goldan, P. D., W. C. Custer, F. C. Fehsenfeld, and S. A. Montzka, Hydrocarbon measurements in the southeastern United States: The rural oxidants in the southern environment (ROSE) program 1990, J. Geophys. Res., 100, 25,94525,963, 1995b.
  • Goldan, P. D., W. C. Custer, and F. C. Fehsenfeld, Nonmethane hydrocarbon measurements during the tropospheric OH photochemistry experiment, J. Geophys. Res., 102, 63156324, 1997.
  • Goode, J. G., et al., Measurements of excess O3, CO2, CO, CH4, C2H4, C2H2, HCN, NO, NH3, HCOOH, CH3COOH, HCHO, and CH3OH in 1997 Alaskan biomass burning plumes by airborne Fourier transform infrared spectroscopy (AFTIR), J. Geophys. Res., 105, 22,14722,166, 2000.
  • Grebe, T. W., and J. Stock, Bacterial chemotaxis: The five sensors of a bacterium, Curr. Biol., 8, R154R157, 1998.
  • Guenther, A., et al., A global model of natural volatile organic compound emissions, J. Geophys. Res., 100, 88738892, 1995.
  • Holmes, M. E., F. J. Sansone, T. M. Rust, and B. N. Popp, Methane production, consumption, and air-sea exchange in the open ocean: An evaluation based on carbon isotopic ratios, Global Biogeochem. Cycles, 14, 110, 2000.
  • Holzinger, R., L. Sandoval-Soto, S. Rottenberger, P. J. Crutzen, and J. Kesselmeier, Emissions of volatile organic compounds from Quercus ilex L. measured by proton transfer fraction mass spectroscopy under different environmental conditions, J. Geophys. Res., 105, 20,57320,579, 2000.
  • Holzinger, R., A. Jordan, A. Hansel, and W. Lindinger, Methanol measurements in the lower troposphere near Innsbruck (47°16′N; 11°24′E), Austria, Atmos. Environ., 35, 25252532, 2001.
  • Iraci, L. T., A. M. Essin, and D. M. Golden, Solubility of methanol in low-temperature aqueous sulfuric acid and implications for atmospheric particle composition, J. Phys. Chem. A, 106, 40544060, 2002.
  • Jacob, D. J., Chemistry of OH in remote clouds and its role in the production of formic acid and peroxymonosulfate, J. Geophys. Res., 91, 98079826, 1986.
  • Jacob, D. J., Heterogeneous chemistry and tropospheric ozone, Atmos. Environ., 34, 21312159, 2000.
  • Jacob, D. J., B. D. Field, E. Jin, I. Bey, Q. Li, J. A. Logan, and R. M. Yantosca, Atmospheric budget of acetone, J. Geophys. Res., 107, 4100, doi:10.1029/2001JD000694, 2002.
  • Jayakumar, D. A., S. W. A. Naqvi, P. V. Narvekar, and M. D. George, Methane in coastal and offshore waters of the Arabian Sea, Mar. Chem., 74, 113, 2001.
  • Jones, R. D., Carbon monoxide and methane distribution and consumption in the photic zone of the Sargasso Sea, Deep-Sea Res., 38, 625635, 1991.
  • Kagan, R. M., H. J. McFadden, P. N. McFadden, C. O'Connor, and S. Clarke, Molecular phylogenetics of a protein repair methyltransferase, Comput. Biochem. Physiol. B, 117, 379385, 1997.
  • Karl, T., A. Guenther, A. Jordan, R. Fall, and W. Lindinger, Eddy covariance measurement of biogenic oxygenated VOC emissions from hay harvesting, Atmos. Environ., 35, 491495, 2001.
  • Kelly, T. J., P. J. Callahan, J. Plell, and G. F. Evans, Method development and field measurements for polar volatile organic compounds in ambient air, Environ. Sci. Technol., 27, 11461153, 1993.
  • Kelly, T. J., R. Mukund, C. W. Spicer, and A. J. Pollack, Concentrations and transformations of hazardous air pollutants, Environ. Sci. Technol., 28, 378A387A, 1994.
  • Kieber, D. J., G. M. Vaughan, and K. Mopper, Determination of formate in natural waters by a coupled enzymatic/high performance liquid chromatographic technique, Anal. Chem., 60, 16541659, 1988.
  • Kieber, R. J., and K. Mopper, Determination of picomolor concentrations of carbonyl compounds in natural waters, including seawater, by liquid chromatography, Environ. Sci. Technol., 24, 14771481, 1990.
  • Kiene, R. P., Microbial sources and sinks for methylated sulfur compounds in the marine environment, in Microbial Growth on C1Compounds: 7, edited by D. P. Kelly, and J. C. Murrell, pp. 1533, Intercept Ltd., London, 1993.
  • Kiene, R. P., and L. P. Hoffmann-Williams, Glycine betaine uptake, retention, and degradation by microorganisms in seawater, Limnol. Oceanogr., 43, 15921603, 1998.
  • Kiene, R. P., L. P. Hoffmann-Williams, and J. E. Walker, Seawater microorganisms have a high affinity glycine betaine uptake system which also recognizes dimethylsulfoniopropionate, Aquat. Microb. Ecol., 15, 3951, 1998.
  • Kiene, R. P., L. J. Linn, and J. A. Bruton, New and important roles for DMSP in marine microbial communities, J. Sea Res., 43, 209224, 2000.
  • King, G. M., M. J. Klug, and D. R. Lovely, Metabolism of acetate, methanol, and methylated amine in intertidal sediments of Love's Cove, Maine, Appl. Environ. Microbiol., 43, 18481853, 1983.
  • Kirstine, W., I. Galbally, Y. Ye, and M. Hooper, Emissions of volatile organic compounds (primarily oxygenated species) from pasture, J. Geophys. Res., 103, 10,60510,619, 1998.
  • Lamanna, M. S., and A. H. Goldstein, In situ measurements of C2−C10 volatile organic compounds above a Sierra Nevada ponderosa pine plantation, J. Geophys. Res., 104, 21,24721,262, 1999.
  • Leibrock, E., and J. Slemr, Method for the measurement of volatile oxygenated hydrocarbons in ambient air, Atmos. Environ., 31, 33293339, 1997.
  • Lelieveld, J., and P. J. Crutzen, The role of clouds in tropospheric photochemistry, J. Atmos. Chem., 12, 229267, 1991.
  • Liang, J., and D. J. Jacob, Effect of aqueous-phase cloud chemistry on tropospheric ozone, J. Geophys. Res., 102, 59936001, 1997.
  • MacDonald, R. C., and R. Fall, Detection of substantial emissions of methanol from plants to the atmosphere, Atmos. Environ., Part A, 27, 17091713, 1993.
  • Milne, P. J., D. D. Riemer, R. G. Zika, and L. E. Brand, Measurement of vertical distribution of isoprene in surface seawater, its chemical fate, and its emission from several phytoplankton monocultures, Mar. Chem., 48, 237244, 1995.
  • Monod, A., and P. Carlier, Impact of clouds on the tropospheric ozone budget: Direct effect of multiphase photochemistry of soluble organic compounds, Atmos. Environ., 33, 44314446, 1999.
  • Monod, A., A. Chebbi, R. Durand-Jolibois, and P. Carlier, Oxidation of methanol by hydroxyl radicals in aqueous solution under simulated cloud droplet conditions, Atmos. Environ., 34, 52835294, 2000.
  • Moore, R. M., and W. Groszko, Methyl iodide distribution in the ocean and fluxes to the atmosphere, J. Geophys. Res., 104, 11,16311,171, 1999.
  • Moore, R. M., W. Groszko, and S. J. Niven, Ocean-atmosphere exchange of methyl chloride: Results from northwest Atlantic and Pacific Ocean studies, J. Geophys. Res., 101, 28,52928,538, 1996.
  • Mopper, K., and D. Kieber, Distribution and biological turnover of dissolved organic compounds in the water column of the Black Sea, Deep Sea Res., 38, S1021S1047, 1991.
  • Mopper, K., and W. L. Stahovec, Sources and sinks of low molecular weight organic carbonyl compounds in seawater, Mar. Chem., 19, 305321, 1986.
  • Mopper, K., and X. Zhou, Photoproduction of hydroxyl radicals at the sea surface and its potential impact on marine processes, in Effects of Solar Ultraviolet Radiation on Biogeochemical Dynamics in Aquatic Environments, edited by N. V. Blough, and R. G. Zepp, Tech. Rep., WHOI-90-09, pp. 151157, Woods Hole Oceanogr. Inst., Woods Hole, Mass., 1990.
  • Nemecek-Marshall, M., R. C. MacDonald, J. J. Franzen, C. L. Wojciechowski, and R. Fall, Methanol emission from leaves. Enzymatic detection of gas-phase methanol and relation of methanol fluxes to stomatal conductance and leaf development, Plant Physiol., 108, 13591368, 1995.
  • Painter, T., Algal polysaccharides, in The Polysaccharides, vol. 2, edited by G. O. Aspenall, pp. 195285, Academic, San Diego, Calif., 1983.
  • Peixoto, J. P., and A. H. Oort, Physics of Climate, Am. Inst. of Phys., New York, 1992.
  • Prinn, R. G., R. F. Weiss, B. R. Miller, J. Huang, F. N. Alyea, D. M. Cunnold, P. J. Fraser, D. E. Hartley, and P. G. Simmonds, Atmospheric trends and lifetime of CH3CCl3 and global OH concentrations, Science, 269, 187192, 1995.
  • Riemer, D., Marine and terrestrial sources of reactive volatile organic compounds and their impact on the tropospheric ozone chemistry of the earth, Ph.D. thesis, Univ. of Miami, Miami, Fla., 1998.
  • Riemer, D., et al., Observations of nonmethane hydrocarbons and oxygenated volatile organic compounds at a rural site in the southwestern United States, J. Geophys. Res., 103, 28,11128,128, 1998.
  • Rinne, H. J. I., A. B. Guenther, C. Warneke, J. A. de Gouw, and S. L. Luxembourg, Disjunct eddy covariance technique for trace gas flux measurements, Geophys. Res. Lett., 28, 31393142, 2001.
  • Sansone, F. J., T. M. Rust, and S. V. Smith, Methane distribution and cycling in Tomales Bay, California, Estuaries, 21, 6677, 1998.
  • Schade, G., and A. Goldstein, Fluxes of oxygenated volatile organic compounds from a ponderosa pine plantation, J. Geophys. Res., 106, 31113124, 2001.
  • Sieburth, J. M., The trophic roles of bacteria in marine ecosystems are complicated by synergistic-consortia and mixotrophic-cometabolism, Prog. Oceanogr., 21, 117128, 1988.
  • Sieburth, J. M., and M. D. Keller, Methylaminotrophic bacteria in xenic nanoalgal cultures: Incidence, significance, and role of methylated algal osmoprotectants, Biol. Oceanogr., 6, 383395, 1989.
  • Sieburth, J. M., P. W. Johnson, M. A. Eberhardt, M. E. Sieracki, M. Lidstrom, and D. Laux, The first methane-oxidizing bacterium from the upper mixing layer of the deep ocean: Methylomonas pelagica sp. nov. Curr. Microbiol., 14, 285293, 1987.
  • Simo, R., C. Pedros-Alio, G. Malin, and J. O. Grimalt, Biological turnover of DMS, DMSP and DMSO in contrasting open-sea waters, Mar. Ecol. Prog. Ser., 203, 111, 2000.
  • Singh, H. B., M. Kanakidou, P. J. Crutzen, and D. J. Jacob, High concentrations and photochemical fate of oxygenated hydrocarbons in the global troposphere, Nature, 378, 5054, 1995.
  • Singh, H. B., et al., Distribution and fate of selected oxygenated organic species in the troposphere and lower stratosphere over the Atlantic, J. Geophys. Res., 105, 37953805, 2000.
  • Singh, H. B., et al., Evidence from Pacific troposphere for large global sources of oxygenated organic compounds, Nature, 410, 10781081, 2001.
  • Snider, J. R., and G. A. Dawson, Tropospheric light alcolhols, carbonyls, and acetonitrile: Concentrations in the southwestern United States and Henry's Law data, J. Geophys. Res., 90, 37973805, 1985.
  • Tsurushima, N., S. Watanabe, and S. Tsunogai, Methane in the East China Sea water, J. Oceanogr., 52, 221233, 1996.
  • Valentine, D. L., D. C. Blanton, W. S. Reeburgh, and M. Kastner, Water column methane oxidation adjacent to an area of active hydrate dissociation, Eel River Basin, Geochim. Cosmochim. Acta, 65, 26332640, 2001.
  • Vaughan, G. M., and K. Mopper, Determination of nanomolar levels of formate in natural waters based on a luminescence enzymatic assay, Anal. Chim. Acta, 231, 299303, 1990.
  • Visscher, P. T., and B. F. Taylor, Demethylation of dimethylpropionate to 3-mercaptoproprionate by an aerobic marine bacterium, Appl. Environ. Microbiol., 60, 46174619, 1994.
  • Ward, B. B., K. A. Kilpatrick, P. C. Novelli, and M. I. Scranton, Methane oxidation and methane fluxes in the ocean surface layer and deep anoxic waters, Nature, 327, 226229, 1987.
  • Ward, B. B., K. A. Kilpatrick, A. E. Wopat, E. C. Minnich, and M. E. Lidstrom, Methane oxidation in Saanich Inlet during summer stratification, Cont. Shelf Res., 9, 6575, 1989.
  • Warneck, P., Chemistry of the Natural Atmosphere, 2nd ed., Academic, San Diego, Calif., 1999.
  • Warneke, C., et al., Acetone, methanol, and other partially oxidized volatile organic emissions from dead plant matter by abiological processes: Significance for atmospheric HOx chemistry, Global Biogeochem. Cycles, 13, 917, 1999.
  • Warneke, C., S. Luxembourg, J. de Gouw, J. Rinne, A. Guenther, and R. Fall, Disjunct eddy covariance measurements of oxygenated volatile organic compounds fluxes from an alfalfa field before and after cutting, J. Geophys. Res., 107, 4067, doi:10.1029/2001JD00594, 2002.
  • Warren, S. G., C. J. Hahn, J. London, R. M. Chervin, and R. Jenne, Global distribution of total cloud cover and cloud type amounts over land, NCAR Tech. Note TN-273+STR, Natl. Cent. for Atmos. Res., Boulder, Colo., 1986.
  • Warren, S. G., C. J. Hahn, J. London, R. M. Chervin, and R. Jenne, Global distribution of total cloud cover and cloud type amounts over the ocean, NCAR Tech. Note TN-317+STR, Natl. Cent. for Atmos. Res., Boulder, Colo., 1988.
  • Wesely, M. L., Parameterization of surface resistances to gaseous dry deposition in regional-scale numerical models, Atmos. Environ., 23, 12931304, 1989.
  • Wesely, M. L., and B. B. Hicks, A review of the current status of knowledge on dry deposition, Atmos. Environ., 34, 22612282, 2000.
  • Williams, J., U. Poschl, P. J. Crutzen, A. Hansel, R. Holzinger, C. Warneke, W. Lindinger, and J. Lelieveld, An atmospheric chemistry interpretation of mass scans obtained from a proton transfer mass spectrometer flown over the tropical rainforest of Surinam, J. Atmos. Chem., 38, 133166, 2001.
  • Yang, X.-H., M. I. Scranton, and C. Lee, Seasonal variations in concentation and microbial uptake of methylamines in estuarine waters, Mar. Ecol. Prog. Ser., 108, 303312, 1994.
  • Yokelson, R. J., et al., Emissions of forlmadehyde, acetic acid, methanol, and other trace gases from biomass fires in North Carolina measured by airborne Fourier transform infrared spectroscopy, J. Geophys. Res., 104, 30,10930,125, 1999.
  • Zafiriou, O. C., Reaction of methyl halides with seawater, J. Mar. Res., 33, 7481, 1975.
  • Zhou, X., and K. Mopper, Photochemical production of low-molecular-weight carbonyl compounds in seawater and surface microlayer and their air-sea exchange, Mar. Chem., 56, 201213, 1997.

Supporting Information

  1. Top of page
  2. Abstract
  3. 1. Introduction
  4. 2. Methanol Sinks Considered
  5. 3. Methanol Sources Reconsidered
  6. 4. Terrestrial Net Fluxes
  7. 5. Summary
  8. Acknowledgments
  9. References
  10. Supporting Information

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