The mechanism for the reaction 2 H₂O₂(aq) $\rightarrow$ 2 H₂O( $\ell$ ) + 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(

\ell

) + 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 is determined by the slow step, which is the rate-determining step. In this mechanism, the slow step involves H₂O₂ and I⁻, so the rate law is Rate = k[H₂O₂][I⁻].

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

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