Chapter 13, Problem 116RQ

Suppose a reaction occurs with the following mechanism:

(1) $2A\stackrel{}{\rightleftharpoons }{A}_2$

(fast)

(2) $A_2+E\stackrel{}{\to }B+C$

(slow)

in which the first step is a very rapid reversible reaction that can be considered to be essentially an equilibrium (forward and reverse reactions occurring at the same rate) and the second is a slow step.

(a) Write the rate law for the forward reaction in step (1).

(b) Write the rate law for the reverse reaction in step (1).

(c) Write the rare law for the rate-determining step.

(d) What is the chemical equation for the net reaction that occurs in this chemical change?

Use the results of parts (a) and (b) to rewrite the rate law of the rate-determining step in terms of the concentrations of the reactants in the overall balanced chemical equation for the reaction.