Chapter 13, Problem 13.5P

(a)

Interpretation Introduction

To determine:

The rate law for this equation.

Interpretation Introduction

To determine the value of ‘y’:

Now, we can compare the rate change in experiment 1 & 3 with respect to the change in the concentration of NO₂and CO both.

$\frac{{[N{O}_2]}_3{}^2*{\left[CO\right]}_3{}^y}{{[N{O}_2]}_1{}^2*{\left[CO\right]}_1{}^y}=\frac{{[0.20]}^2*{[0.20]}^y}{{[0.10]}^2*{[0.10]}^y}=4*{\left(2\right)}^y=\frac{{[Rate]}_3}{{[Rate]}_1}=\frac{2*{10}^{-2}}{5*{10}^{-3}}=4$

Taking logarithm both the side-

$Log\left(4*2^y\right)=Log(4)$

$2Log\left(2\right)+yLog(2)=2Log\left(2\right)$

So $x=\frac{0}{0.3}=0$

So the order of reaction in CO is 0
That means the reaction don’t depend on the concentration of CO.

So, the final rate law is −
Rate = $k*{\left[N{O}_2\right]}^2*{\left[CO\right]}^0$

(b)

Interpretation Introduction

To determine:

To determine the value of rate constant and its units.

(c)

Interpretation Introduction

To determine:

To determine rate of consumption of NO₂in the given condition.