Be sure to answer all parts. The catalytic destruction of ozone occurs via a two-step mechanism, where X can be any of several species: (1) X + O3 → XO + O2 [slow] (2) XO + O → X + O2 [fast] (a) Write the overall reaction. O3 + XO → X + 2 O2 X + O3 → XO + O2 XO + X + O3 + O → XO + X + 2 O2 O3 + O → 2 O2 (b) Write the rate law for each step (using k for the rate constant). Reaction 1: Reaction 2: k[X][O3] k[XO][O2] k[X][O2] k[XO][O3] k[XO][O2] k[X][O] k[X][O2] k[XO][O] (c) X acts as a and XO acts as a catalyst intermediate catalyst intermediate (d) High-flying aircraft release NO into the stratosphere, which catalyzes the process. When O3 and NO concentrations are 9 × 1012 molecule/cm3 and 7.4 × 109 molecule/cm3, respectively, what is the rate of O3 depletion