Chemistry

Problem

The reaction :

2A \rightarrow 2B + C

occurs by the mechanism :

A \xrightarrow{k_1} B + X \text{ (slow)} \quad \dots\dots\dots (1)

A + X \xrightarrow{k_2} B + C \text{ (fast)} \quad \dots\dots\dots (2)

Which of the following step is incorrect ? (A) Molecularity of the reaction is one (B) The order of the reaction with respect to A is two (C) The rate law is :

v = k_1 [A]

(D)

k_2 > k_1

Browse the problem library