Question

The rate determining step for the destruction of ozone is the formation of the Clo dimer (formula: CloOCI) shown in the equation below. The rate is second order to the concentration of Clo. ClO+ CIO ooc (kaea3.4x1012 molecule cm s) This reaction is followed by the fast photolysis of the dimer and the fast destruction of ozone by Cl atoms: CLOOC+hy 2 CI+O Given the following concentrations: [CIO] 9.8 x 10 molecule cm and initial O, concentration 1 x 10 molecule cm I using the provided initial concentration of ozone, determine the time (in days) required to deplete 90 % of ozone assuming ozone is not replenished by sunlight.

Answer 1

Comment in case of any doubt.

Overall reaction can be written as 240 +20~240 +292 liven reaction is second order in co. For every turo co, two Ę are used So, rate of destruction of O cante twice of the rate of reaction. Tale of rxn is: written as 8 = K[o]² So 3 dC0p] = K[UD] => [027-2x [CRO] But eo acts only as catalyst, so [co] will be constant and equal to 9.8*10% molecule com? Thes, de -2 (3-4xjö?malecelias 1) (918x10% malesuada >> DCOM] =* 6.50072 xvó melalui Jargs [-6:53072 x 6 matemati) at | 2 - 0 9 0 x 2 = -6, S70 72 A) pºt 0.10X10 Iday -) t = 1378.02 seconds x Imin x than to second Gomin 24h = [0.16 day = 0 Answer swer