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3 ppm chemistry o3 reactions o2 hv o o photolysis

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Unformatted text preview: 1/25 the density of air we breathe (more dilute) We are talking about ozone depletion in stratosphere (not ozone smog in troposphere) Absorbs low wavelength UV photons that would damage a lot of stuff on earth if not contained Stratospheric Photochemistry in Nature (without human intervention) Ozone is naturally created and destroyed to create a stable equilibrium concentration in the atmosphere (0.3 ppm) Chemistry: O3 reactions O2 + hv O + O (photolysis) O + O2 + N2 O3 + N2 (O3 formation) Light: N2 only absorbs energy and heats stratosphere, chemically inactive. The higher you go the warmer it gets because of this. O3 + hv O + O2 (O3 photolysis) OR it can O + O3 O2 + O2 Chlorofluorocarbons (CFC’s) Used in a lot of common- day products Carbons with Cl and F Every single pound of CFC created stayed in the stratosphere for about a hundred years. Rowland and Molina’s Reactions: C2Cl5F + UV Cl + C2Cl4F (in the upper stratosphere Cl + O3 ClO + O2 ClO + O Cl + O2 (Cl regeneration, so destruction of even more ozone) O + O3 O2 + O2 NET: O + O3 O2 + O2 Cl can be reused over 100,000 times. Cl is a catalyst. Terminates when Cl + NO2 ClONO From this you can predict a change in the equilibrium ratio of O2 and O3 in the stratosphere Three different phenomena: CFC’s destr...
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