The mechanism for the reaction 2 H₂O₂ (aq) $\rightarrow$ 2 H₂O(l) + O₂(g) in the presence of I^-(aq) is proposed to be:
Step 1: H₂O₂(aq) + I^-(aq) $\rightarrow$ H₂O(l) + OI^-(aq) (slow)
Step 2: H₂O₂(aq) + OI^-(aq) $\rightarrow$ H₂O(l) + O₂(g) +I^-(aq) (fast) What is the rate law for the overall reaction?

Question

The mechanism for the reaction 2 H₂O₂ (aq)

\rightarrow

2 H₂O(l) + O₂(g) in the presence of I^-(aq) is proposed to be:
Step 1: H₂O₂(aq) + I^-(aq)

\rightarrow

H₂O(l) + OI^-(aq) (slow)
Step 2: H₂O₂(aq) + OI^-(aq)

\rightarrow

H₂O(l) + O₂(g) +I^-(aq) (fast) What is the rate law for the overall reaction?

Quizplus · Accepted Answer

The rate law for a reaction is determined by its slowest step, because the slowest step is the rate-determining step. In this proposed mechanism, Step 1 is the slow step, and it involves one molecule of H₂O₂ and one molecule of I^{F1F1F1S1uf02dF1F1F10} reacting together. Therefore, the rate law is proportional to the concentrations of these two reactants, which is option C: k[H₂O₂][I^{F1F1F1S1uf02dF1F1F10}].

The Mechanism for the Reaction 2 H2O2 (Aq) →\rightarrow→ 2 H2O(l) + O2(g) in the Presence of I-(aq) Is

The Mechanism for the Reaction 2 H₂O₂ (Aq) $\rightarrow$ 2 H₂O(l) + O₂(g) in the Presence of I^-(aq) Is