Chapter 14, Problem 14.69SP

Interpretation Introduction

(a)

Interpretation:

The rate law needs to be determined.

Concept introduction:

Consider the general reaction,

$\text{aA+bB}\to \text{Products}$

Here, A and B are reactants and a, b are stoichiometric coefficients in the balanced chemical reaction. Rate law of the above reaction is as follows:

$\text{Rate}\text{=}k{\left[\text{A}\right]}^m{\left[\text{B}\right]}^n$

Here, k represents rate constant and m, n represents order with respect to A and B.

Interpretation Introduction

(b)

Interpretation:

The initial rate needs to be determined, when the initial concentration of $\left[{\left({\text{CH}}_{\text{3}}\right)}_{\text{3}}\text{N}\right]$ is $4.2\times {10}^{-2}\text{M}$ and $\left[{\text{ClO}}_{\text{2}}\right]$ is $3.4\times {10}^{-2}\text{M}$.

Concept introduction:

Consider the general reaction

$\text{aA+bB}\to \text{Products}$

Here, A and B are reactants and a, b are stoichiometric coefficients in the balanced chemical reaction. Rate law of the above reaction is as follows:

$\text{Rate}\text{=}k{\left[\text{A}\right]}^m{\left[\text{B}\right]}^n$

Here, k represents rate constant and m, n represents order with respect to A and B.