Chapter 16, Problem 78A

Interpretation Introduction

Interpretation:

To calculate the average reaction rate during the time interval if the concentration of a reaction product increases from 0.0882 mol/L to 0.1446 mol/L in 12.0 minutes.

Concept introduction:

In a chemical reaction, the reactants are written on the left side of the equation and the product is written on the right side.

The average rate of a reaction can be given by the formula,

Average reaction rate $\text{=}-\frac{\text{Δ}\left[\text{reactant}\right]}{\text{Δt}}$

Here, $\text{Δ}\left[\text{reactant}\right]$ = change in the concentration of the reactant

Answer to Problem 78A

The average reaction rate during the time interval if the concentration of a reaction product increases from 0.0882 mol/L to 0.1446 mol/L in 12.0 minutes is $0.0470\frac{\text{mol}}{\text{L}\text{.min}}$

Explanation of Solution

Given, the concentration of a reaction increases from 0.0882 mol/L to 0.1446 mol/L in 12.0 min. So, the change in time is $\Delta t=12.0\min$ and the change in the concentration is $\text{Δ}\left[\text{product}\right]\text{=}\text{0}\text{.1446}\text{mol/L}-\text{0}\text{.0882}\text{}\text{mol/L}$. Using these values, we calculate the value of average reaction rate.

$\text{Average reaction rate =}\frac{\text{Δ}\left[\text{product}\right]}{\Delta t}$

$\begin{array}{l}\text{=}\frac{\text{0}\text{.1446}\text{mol/L}-\text{0}\text{.0882}\text{}\text{mol/L}}{12.0\min }\\ =\frac{0.0564}{12.0}\frac{\text{mol}}{\text{L}\text{.min}}\\ =0.0470\frac{\text{mol}}{\text{L}\text{.min}}\end{array}$

Therefore, the average reaction rate during the given time interval is $0.0470\frac{\text{mol}}{\text{L}\text{.min}}$

Conclusion

The average reaction rate during the time interval is $0.0470\frac{\text{mol}}{\text{L}\text{.min}}$