Chapter 16.4, Problem 39SSC

Interpretation Introduction

Interpretation:

The rate of reaction for the reaction between A and B needs to be determined with the help of given information.

• Order with respect to A = 1
• Order with respect to B = 1
• Rate constant = 0.500 mol/L.s
• [A] = 2.00 x 10-2 M
• [B] = 1.50 x 10-2 M

Concept introduction:

Chemical kinetic is the branch of chemistry that deals with kinetic or rate of a chemical reaction. The rate of reaction can be defined as the change in the concentration of reactant and product with time. The rate of reaction mainly depends on the activation energy.

Answer to Problem 39SSC

$\text{Rate = }1.5{\text{ × 10}}^{\text{-4}}{\text{ M}}^{\text{3}}\text{/sec}$

Explanation of Solution

Given information:

• Order with respect to A = 1
• Order with respect to B = 1
• Rate constant = 0.500 mol/L.s
• [A] = 2.00 x 10-2 M
• [B] = 1.50 x 10-2 M

The rate law must be written as:

$\text{Rate = k [A] [B] }$

Substitute the values to calculate the rate:

$\begin{array}{l}\text{Rate = k [A] [B] }\\ \text{Rate = 0}\text{.500 mol/L}\text{.s [2}\text{.00}\times {\text{10}}^{\text{-2}}\text{M] [1}\text{.50}\times {\text{10}}^{\text{-2}}\text{M]}\\ \text{Rate = }1.5{\text{ × 10}}^{\text{-4}}{\text{ M}}^{\text{3}}\text{/sec}\end{array}$

Conclusion

Thus,

$\text{Rate = }1.5{\text{ × 10}}^{\text{-4}}{\text{ M}}^{\text{3}}\text{/sec}$