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

Question

Quizplus · Accepted Answer

The rate law is determined by the slowest step, which is Step 1. According to the stoichiometry of the slowest step, the rate depends on the concentrations of [H₂O₂] and [I^-]. Thus, the rate law is given by k[H₂O₂][I^-]. The concentration of the product [OI^-] is not included in the rate law as it is formed in Step 2, which is a fast step and does not contribute significantly to the rate of the overall reaction. Choice A, B, D, and E do not correctly represent the rate law for the given mechanism.

The Mechanism for the Reaction 2 H2O2(aq) →\to→ 2 H2O( )+ O2(g)in the Presence of I-(aq)is Proposed

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