Chemistry

Chemistry

Problem

The decomposition of ozone in the stratosphere can proceed via the following two-step mechanism: Step 1 (slow): Cl(g)+O3(g)→ClO(g)+O2(g)\text{Cl}(g)+\text{O}_3(g)\rightarrow\text{ClO}(g)+\text{O}_2(g) Step 2 (fast): ClO(g)+O(g)→Cl(g)+O2(g)\text{ClO}(g)+\text{O}(g)\rightarrow\text{Cl}(g)+\text{O}_2(g) What is the predicted rate law for the overall reaction based on this mechanism? a) rate = k[ClO][O]k[\text{ClO}][\text{O}] b) rate = k[Cl][O3]k[\text{Cl}][\text{O}_3] c) rate = k[Cl]2[O3]k[\text{Cl}]^{2}[\text{O}_3] d) rate = k[O][O3]k[\text{O}][\text{O}_3]

Browse the problem library