Chapter 18, Problem 18.73P

Interpretation Introduction

Interpretation:

Using the steady – state approximation for $\left[A^{*}\right]$, the rate law for the overall reaction has to be derived.

  $Rateofreaction=-\frac{\Delta \left[A\right]}{\Delta t}=\frac{k_1{k}_2\left[A\right]\left[M\right]}{k_{-1}\left[M\right]+k_2}$

Concept Introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

  $\begin{array}{l}\text{aA + bB}\to x\text{X}\\ \\ {\text{Rate of reaction = k [A]}}^{\text{m}}{\text{[B]}}^{\text{n}}\\ \\ \text{Total}\text{order}\text{of reaction = }\left(\text{m + n}\right).\end{array}$

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

Steady – state approximation:

Steady – state approximation is applicable on an intermediate.  At steady – state approximation, the rate of formation is equal to the rate of decomposition.