Asked by Jason
Ozone, O3, absorbs ultraviolet radiation and dissociates into O2 molecules and O atoms:
O3 + hv --> O2 + O
A 1.10 L sample of air at 22 degrees Celsius and 748mm Hg contains 0.25ppm of O3.
How much energy, in joules, must be absorbed if all the O3 molecules in the sample of air are to dissociate? Assume that each photon absorbed causes one O3 molecule to dissociate, and that the wavelength of the radiation is 254 nm
O3 + hv --> O2 + O
A 1.10 L sample of air at 22 degrees Celsius and 748mm Hg contains 0.25ppm of O3.
How much energy, in joules, must be absorbed if all the O3 molecules in the sample of air are to dissociate? Assume that each photon absorbed causes one O3 molecule to dissociate, and that the wavelength of the radiation is 254 nm
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