Introduction into Atmospheric Chemistrylpc2e.cnrs-orleans.fr/~specatmos/documents... · Source:...
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Introduction into Atmospheric Chemistry
Christa Fittschen
June 12, 2017 Christa Fittschen 1
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• Introduction to Atmospheric Composition and Pollution Phenomena
• Composition and structure of the Atmosphere
• Key trace gases in Atmospheric Chemistry
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Brief History of Air pollution
Long long time ago … First pollution event during the Roman Empire
“Greek and Roman lead and silver mining and smelting activities polluted the middle troposphere “ (Hong et al, 1994)
From ice cores analyses
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End of the 19th Century: Industrial Revolution
(Source: M. Pidwirny)
Intense use of fossil fuels ⇒ Emission of pollutants (CH4, CO2)
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At the same period, ozone concentration increases …
• Ozone is a secondary pollutant, produced by photochemical processes involving primary pollutants
• Ozone concentration has been increased by a factor of 5 since the late 19th Century
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• Introduction to Atmospheric Composition and Pollution Phenomena
• Composition and structure of the Atmosphere
• Key trace gases in Atmospheric Chemistry
- London smog
- L.A. smog
- Global Troposheric pollution
- Particles
- Acid deposition
- Stratospheric Ozone depletion
- Global Climate Change
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Interest in atmospheric composition
Climate Change (…1990s…)
Regional Air Pollution (…1950s…)
Acid rain (1970s…)
Stratospheric Ozone depletion
(1985…)
Atmospheric CHEMISTRY
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Jacobson et al., Atmospheric pollution
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Youngstown, Ohio (c. 1910)
Reading, Pennsylvania (c. 1909)
Gary, Indiana (c. 1912)
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Noontime, Donora, Pennsylvania, October 29, 1948
Copyright Photo Archive/Pittsburgh Post-Gazette, 2001. All rights reserved
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Pedestrians in Los Angeles (1950s)
M. Jacobson, Air pollution
Los Angeles (July 23, 2000)
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Arie Haagan-Smit demonstrates smog formation. (undated photo, Caltech Archives)
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Ozone pollution has become commonplace
Ozone concentration in µg/m3 (8th August 2003)
Number of hours the threshold value of 180µg/m3 was exceeded (1-14 August 2003)
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Ozone trend from European mountain observations, 1870-1997
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Air Pollution and Visibility
Pictures taken from a same location, at same time of day, on two different days (source: Qi Zhang)
Reduction of visibility by aerosols
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Visibility reduction due to particles Bryce Canyon Great Smokies NP
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Acid rain
Getting better in the U.S.
… but worsening in Asia
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Stratospheric ozone depletion observed in the 80’s
Data from NASA (TOMS instrument) June 12, 2017 Christa Fittschen 28
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Rowland, Molina and Crutzen (1974)
• Discovered that CFCs can last 10-100s of years in atmosphere
• CFCs are susceptible to break down by UV
• Predicted that CFCs will reduce ozone inventories
• Proof that this was occurring came in 1985
• Montreal Protocol 1987
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• Absorption of UV light is sufficiently energetic to cause a photochemical reaction in which the DNA breaks down
Effect of UV Light on DNA
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Absorption Spectrum of DNA • Each of the base pairs have slightly different
absorption spectra
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Absorption Spectrum of DNA • The absorption spectrum of DNA is an average of the
spectra of its base pairs with a peak near 260 nm
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• It is the UV-B region where DNA will absorb UV light
Absorption Spectrum of DNA • In the UV-C region virtually no UV light
reaches the earth’s surface
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• The UV-B region will expand as there will be insufficient ozone to remove all the UV light
Effect of Ozone Depletion
• 1-2% increase in skin cancer for each 1% decrease in ozone
• Currently, one in five Americans will develop skin cancer in their lifetime
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Large increases in greenhouse gases and aerosols since pre-industrial times
Climate change
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Date Speaker / Intervenant 37
Scales of air pollution
Local pollution (urban and industrial) - Primary pollutants: NOx, VOCs, PAHs, dioxines… - Time scale: 1h - 1 week
Regional and continental pollution - Secondary pollutants: NO2, tropospheric O3, CO, acid rains - Time scale: 1 day - 1 month
Global pollution - Long-life trace species : CO2, CH4, N2O, SF6, CFCs, …
- Time scale: few months - 100 years
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• Introduction to Atmospheric Composition and Pollution Phenomena
• Composition and structure of the Atmosphere
• Key trace gases in Atmospheric Chemistry
-Temperature and Pressure structure of the Atmosphere
-Chemical composition of the Atmosphere
- Different sources of Traces Gases
- Transport and Distribution of Traces Gases
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Atmosphere is very thin...
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Atmospheric Structure
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Temperature structure • In absence of local heating, T decreases with
height • Exceptions: Stratosphere: Chapman Cycle (1930s) O2 + hν → 2 O O + O2 (+ M) → O3 (+ heat) O + O3 → 2 O2 (+ heat) O3 + hν → O + O2 • Why is there an ozone “layer”? • Inversion layers are stable: no vertical motion • Tropopause is coldest region: no transport of
condensable molecules (H2O)
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Pressure structure • Scale height H(z) = RT(z) / M x g • Dalton’s law: each component behaves as if it was
alone in the atmosphere • H(z) depends on mass M - O2 lower than N2?? • No, gravitational separation much slower than
turbulent diffusion - only at > 100km enriched in lighter gases • H = 8.5km at 290 K, 6 km at 210 K • 99% of atmospheric mass is below 50km
(troposphere + stratosphere)
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Definitions Mixing ratio:
Volume mixing ratio:
number of moles(A)/number of moles(air) = molecules(A)/molecules(air).
Units: ppmv = 10-6 mole/mole (parts per million) ppbv = 10-9 mole/mole (parts per billion)
Attention with the word billion: can be 109 or 1012 !!! ppt = 10-12 mole/mole (parts per trillion)
Mass mixing ratio: mass(A)/mass(air)
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Atmospheric Composition
Nitrogen
Oxygen
H2O Argon
20%
78%
1%
N2O 310
H2
CO
Ozon
500
100
30 ppb
CO2
CH4 (1.8)
ppm
380
Ne
18 He (5)
HCHO 300
Ethane
SO2 NOx
500
200 100
ppt
NH3 400
CH3OOH 700
H2O2 500
HNO3 300
others
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TRANSPORT of gases
Source: Introduction to Atmospheric Chemistry, Jacob, D. J., 1999
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Residence times and spatial variability
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• Introduction to Atmospheric Composition and Pollution Phenomena
• Composition and structure of the Atmosphere
• Key trace gases in Atmospheric Chemistry
- Hydroxyl radical (OH)
- Reactive nitrogen species
- Hydrocarbons
- Ozone
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Some important Trace gases
• Hydroxyl radical (OH)
• Reactive nitrogen species
• Hydrocarbons
• Ozone
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troposphere
stratosphere
CO
H2O,O3 OH
CO
CO2
View prior to 1970s: Inert troposphere (only source of oxidants in the stratosphere)
With an inert troposphere: With increasing emissions from fossil fuel combustion will CO accumulate in the troposphere?
View of an inert troposphere challenged [Weinstock, 1969]: 14CO measurements in troposphere imply a 2-month lifetime for CO there MUST be a tropospheric sink!
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Primary source of tropospheric OH [Levy, 1971] O3 + hν O2 + O(1D) 290 nm <λ<330 nm O(1D ) + M O(3P) + M M (“third body”) = O2 or N2 O(3P) + O2 + M O3 + M O(1D) + H2O OH + OH
2 OH Solar radiation (290<λ<330 nm)
(~1%)
(~99%)
~1% Only 10% of total O3 are found in the troposphere!
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Sinks of OH Dominant sinks of OH in the global troposphere: 70%: CO + OH CO2 + H 30%: CH4 + OH CH3 + H2O …CO Over continents, reactions with non-methane hydrocarbons (NMHCs) dominates: NMHC + OH products Lifetime of OH ~ 1 second!
CO
CH4
CO NMHCs
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Has human activities changed the oxidizing capacity of the atmosphere?
Since pre-industrial times CO has increased by factors of 3-4; NO has increased by factors of 2-8 …. What has happened to OH?
NO ↑ increase in OH CO ↑ decrease in OH
troposphere
OH HO2 hν, H2O
NO O3
CO, hydrocarbons
Wang & Jacob, 1999
Increase in OH near sources driven by increases of NOx (~days)
Decrease in OH away from sources driven by increases of CO (~months) Little change in OH
globally (buffering)
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Some important Trace gases
• Hydroxyl radical (OH)
• Reactive nitrogen species
• Hydrocarbons
• Ozone
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Reactive nitrogen species and the nitrogen cycle
• Molecular nitrogen: N2 , 78% (~99.99% of all nitrogen) • Nitrous oxide: N2O, 310 ppmv • Reactive nitrogen species: NOy (pptv-ppbv) NOy = NO+NO2(=NOx) + NO3+N2O5+HNO3+ PAN
(=CH3C(O)OONO2) • Ammonia: NH3 pptv-ppbv
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The crucial role of NOx
The catalytic ozone formation cycle NO + O3 → NO2 + O2 NO2 + hν + O2 → NO + O3
NO + HO2 → NO2 + OH NO + CH3O2 → NO2 + CH3O these are the key reactions! NO + RO2 → NO2 + RO
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NO2 NO + O3
hν
Unperturbed cycle leads to
equilibrium concentration of
NO2 / NO / O3
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The crucial role of NOx
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Net formation of 1 molecules O3
Net formation of 2 molecules O3
hν
OH
NO2 NO + O3
hν
HO2
NO2 NO
hν
RO
NO NO2
hν O3
RO2
Hydrocarbons - biogenic - anthropogenic
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The crucial role of NOx
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OH
hν NO2 NO + O3
hν
HO2
NO2 NO
hν
RO
NO NO2
hν O3
RO2
Hydrocarbons - biogenic No NOx is available
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Change in chemistry between “polluted” and “clean” atmospheres
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Change in chemistry between “polluted” and “clean” atmospheres
OH HO2
RO2
Hydrocarbons - biogenic
+ → mostly stable products
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1015 cm-2
Tropospheric NO2 columns from the GOME satellite
August 2000
Concentration of NOx
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Some important Trace gases
• Hydroxyl radical (OH)
• Reactive nitrogen species
• Hydrocarbons
• Ozone
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Methane, CH4
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Fluxes in TgC/year
COCO2
Historical methane trend
Anthropogenic sources: ~70%
The budget of CH4
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Nonmethane hydrocarbons Alkanes (C-C single bonds) Alkenes (C-C double bonds)
ethene ethane
Alkynes (C-C triple bonds)
ethyne Benzene
Aromatic compounds
Oxygenated hydrocarbons: Aldehydes, alcohols, ketones, etc…
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Global emissions of non-methane hydrocarbons ANTHROPOGENIC SOURCES ~100 TgC/yr Energy use and transfer 43 TgC/yr Biomass burning 45 TgC/yr Organic solvents 15 TgC/yr NATURAL SOURCES ~1170 TgC/yr Emissions from vegetation isoprene (C5H8) 500 TgC/yr monoterpenes 125 TgC/yr other VOC 520 TgC/yr Oceanic emissions 6-36 TgC/yr
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Satellite observations of HCHO Hours/ days
Hours/ days
HCHO NMHC CO
OH
Isoprene emissions
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CxHy + (x + 0.25y) O2 x CO2 + H2O y 2
Fate of organic carbon : what says thermodynamics ?
[CH4] = 1.8 ppm
[CO2] = 370 ppm [CO2] ≈ 102 [CH4]
Atmospherique concentrations of CO2 et CH4 :
Kinetic limitations !
Atmosphere = oxidizing environment H → H2O ; N → HNO3 ; S → H2SO4
∆G° ≈ -800 kJ/mol
K= [CO2][H2O]2
[CH4][O2]2 ≈ 10140 At equilibrium : [CO2] ≈ 10144 [CH4]
Oxydation of organique carbon is complet
Example : atmospheric combustion of methane
CO2 + 2 H2O CH4 + 2 O2
C → CO2
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Bond energy - collision energy
For CH4 : ECH3-H = 435 kJ/mol For O2 : EO=O = 492 kJ/mol
Collision energy Photon energy
Ecollision ≈ 3 kJ/mol E300 nm ≈ 400 kJ/mol
Bond energy :
Collisions between CH4+O2 are not « energetic » enough to break the bond
No reaction between CH4 and O2
How do they get over the barrier??
In the stratosphere : O2 + hν (λ < 240 nm) 2 O
In the troposphere : catalytiques (photochemical) cycles
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Tropospheric OH production takes place in a narrow UV window (300-320 nm)
30o equinox midday Solar spectrum
λ300nm= 400 kJ mol-1
λ400nm= 300 kJ mol-1
O-NO=306 kJ mol-1
O-OO=105 kJ mol-1
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Carbon monoxide, CO
CH4 CO2
Fluxes in TgC/year
CO sources: ~25% Fossil fuel, ~25% Biomass burning ~25% CH4 oxidation, ~25% NMHC oxidation
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Some important Trace gases
• Hydroxyl radical (OH)
• Reactive nitrogen species
• Hydrocarbons
• Ozone
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Transport from the Stratosphere: 475 Tg/yr
Deposition: 1165 Tg/yr
Chemically produces in the Troposphere: 4920 Tg/yr
Chem loss: 4230 Tg/yr
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Ozone concentration is measured in Dobson units
All the Ozone over a certain area is compressed down to 0°C and 1 atm pressure. A slab of 1mm thick corresponds to 100 DU.
O3 Area covered by Column
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Tropospheric ozone column seen from space
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Historical records imply a large anthropogenic contribution to the present-day ozone background at northern midlatitudes
Ozone trend from European mountain observations, 1870-1990
[Marenco et al.,1994]
Increase is important from pollution and climate perspectives
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Some important Trace gases
• Hydroxyl radical (OH)
• Reactive nitrogen species
• Hydrocarbons
• Ozone
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Lab studies
Modeling Atmosphere’s observations
Provide data + validation of 0D models Help for the
definition of the experiments
Help for the preparation of field campains
Validation of chemical-transport models (3D)
Identification of new species
Identification of new species
How to study atmospheric chemistry?
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Lab studies
• Provide kinetic and mechanistic data in order to:
– Identify major reactions
– Determine lifetimes of trace species
– Identify oxidation products, which can themselves affect air quality or play an important role in atmospheric chemistry
– Provide data for chemical schemes in models
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Thank you very much for your
attention!!
Any questions??
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