Atmospheric chemistry Day 2 Stratospheric chemistry.
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Transcript of Atmospheric chemistry Day 2 Stratospheric chemistry.
UV absorption spectrum of O3 at 298 K
Small but significant absorption out to 350 nm (Huggins bands)
Hartley bands
Very strong absorption
Photolysis mainly yields O(1D) + O2, but as the stratosphere is very dry (H2O ~ 5 ppm), almost all of the O(1D) is collisionally relaxed to O(3P)
At the ground [O3] ~ 10-100 ppb, in the stratosphere [O3] ~ 5-10 ppm
O3 altitude profile measured from satellite
Total column amount of ozone measured by the Total Ozone Mapping Spectrometer (TOMS)
instrument as a function of latitude and season
Can we account for the distribution of ozone?
J1 = rate of O2 photolysis (s-1)
J3 = rate of O3 photolysis (s-1)
Graph shows the altitude dependence of the rate of photolysis of O3 and O2. Note how J1 is very small until higher altitudes
(1) The ratio J1/J3 increases rapidly with altitude, z
(2) As pressure exp (-z) then [O2]2 [M] decreases rapidly with z
z][][][ 2
24
2
3
13 MO
k
k
J
JO
This balance results in a layer of O3
Altitude/km
J1J3
J1
J3
The Chapman mechanism overpredicts O3 by a factor of 2.
Something else must be removing O3
(Or the production is too high, but this is very unlikely)
Alt
itu
de
/ km
HOW GOOD IS THE CHAPMAN MECHANSIM?
Catalytic ozone destructionThe loss of odd oxygen can be accelerated through catalytic cycles whose net result is the same as the (slow) 4th step in the Chapman cycle
Uncatalysed: O + O3 O2 + O2 k4
Catalysed: X + O3 XO + O2 k5
XO + O X + O2 k6
Net rxn: O + O3 O2 + O2
X is a catalyst and is reformed
X = OH, Cl, NO, Br (and H at higher altitudes)
Reaction (4) has a significant barrier and so is slow at stratospheric temperatures
Reactions (5) and (6) are fast, and hence the conversion of O and O3 to 2 molecules of O2 is much faster, and more ozone is destroyed.
Using the steady-state approximation for XO, R5=R6 and hence k5[X][O3] = k6[XO][O]
Rate (catalysed) / Rate (uncatalysed) = R5/R4 = k5[X][O3]/k4[O][O3]= k5[X]/k4[O]
Or Rate (catalysed) / Rate (uncatalysed) = R6/R4 = k6[XO][O]/k4[O][O3]=k6[XO]/k4[O3]
Note that rate coefficients for X+O3 (k5) and XO+O (k6) are much higher than for O + O3 (k4) So don’t need much X present to make a difference
k5 k6
k4
CFC’s are not destroyed in the troposphere. They are only removed by photolysis once they reach the stratosphere.
Data from NOAA CMDL
Ozone depleting gases measured using a gas chromatograph with an electron capture detector (invented by Jim Lovelock)
These are ground-based measurements. The maximum in the stratosphere is reached about 5 years later
45 years 100 years
Why are values in the N hemisphere slightly higher?
“Do nothing” cycles
Ox is not destroyed
Reduces efficiency of O3 destruction
Removal of the catalyst X. Reservoir is unreactive and relatively stable to photolysis. X can be regenerated from the reservoir, but only slowly. [X] is reduced by these cycles.
For Cl atom, destroys 100,000 molecules of O3 before being removed to form HCl
Interactions between different catalytic cycles
Reservoir species limit the destruction of ozone
ClONO2 stores two catalytic agents – ClO and NO2
Effects of catalytic cycles are not additive due to coupling
Mechanism Ozone Column
(Dobson units)
Chapman only (C) 644
C + NOx 332
C + HOx 392
C + ClOx 300
C + NO x+ HOx + ClOx 376
Coupling to NO leads to null cycles for HOx and ClOx cycles
Increase of Cl and NO concentrations in the atmosphere has less effect than if Cl or NO concentrations were increased separately
(because ClOx and NOx cycles couple, hence lowering [X])
Bromine cycle
Br + O3 BrO + O2
Cl + O3 ClO + O2
BrO + ClO Br + ClOO
ClOO Cl + O2
Net 2O3 3 O2
Br and Cl are regenerated, and cycle does not require O atoms, so can occur at lower altitude
Source of bromine : CH3Br (natural emissions from soil and used as a soil fumigant)
Halons (fire retardants)
Catalytic cycles are more efficient as HBr and BrONO2 (reservoirs for active Br) are more easily photolysed than HCl or ClONO2
But, there is less bromine than chlorine
Bromine is very important for O3 destruction in the Antarctic stratosphere where [O] is low
TOMS (on Nimbus 7 satellite)
o Dobson spectrophotometer
October ozone column, Halley Bay, Antarctica
Total Ozone Mapping Spectrometer (TOMS)
Monthly October averages for ozone, 1979, 1982, 1984, 1989, 1997, 2001
Dobson units (total O3 column)
October 2000 “For the Second time in less than a week dangerous levels of UV rays bombard Chile and Argentina, The public should avoid going outside during the peak hours of 11:00 a.m. and 3:00 p.m. to avoid exposure to the UV rays”
Ushaia, Argentina
The most southerly city in the world
At 15 km, all the ozone disappears in less than 2 months
This cannot be explained using gas-phase chemistry alone
US Base in Antarctica
Simultaneous measurements of ClO and O3 on the ER-2
Late August 1987 September 16th 1987
The “smoking gun” experiment – proved the theory was OK
Still dark over Antarctica Daylight returns
Simultaneous measurements of ClO and O3 on the ER-2
Late August 1987 September 16th 1987
The “smoking gun” experiment – proved the theory was OK
Still dark over Antarctica Daylight returns