Chapter 6, Problem 6.10DQ

Interpretation Introduction

Interpretation:

The pre equilibrium and steady-state approximations have to be specified and the reason for why they might lead to different conclusions has to be explained.

Concept Introduction:

Chemical equilibrium: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.

Steady state approximation: This method used to derive a rate law. The method is based on the assumption that one intermediate in the reaction mechanism is consumed as quickly as it is generated.

Example: Use the SSA approximate to calculate the concentration of the intermediate $\left(C\right)$ in the following sequence of elementary steps.

  $\begin{array}{l}A+B\underset{k_2}{\overset{k_1}{\rightleftharpoons }}C\\ C\stackrel{k_2}{\to }D\end{array}$

Where the rate constant $\left(k_r\right)$ is indicated, the overall reaction is.

$A+B\stackrel{}{\to }D$