Chapter 17, Problem 60A

Interpretation Introduction

Interpretation:

By changing the volume of the system, the change in equilibrium of the given reactions needs to be explained.

Concept introduction:

The equilibrium state is the state where the concentration of reactants and products becomes equal.

Answer to Problem 60A

In the reaction $\left(\text{A}\right)$, the equilibrium shifts towards the reactants side due to the change in volume f the system because numbers of moles are greater on reactants side as compared to that of products.

In the reaction $\left(\text{B}\right)$, there is no effect on the equilibrium state because there are equal number of molecules on both side of the reaction.

Explanation of Solution

The given reactions are

${\text{N}}_{\text{2}}\left(\text{g}\right){\text{+3H}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{2NH}}_{\text{3}}\left(\text{g}\right)$, and

${\text{H}}_{\text{2}}\left(\text{g}\right){\text{+Cl}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons \text{2HCl}\left(\text{g}\right)$

In the first reaction, number of molecules on reactant side is greater than that of product. So, by changing the volume of the system, the equilibrium shifts towards the left side.

Similarly, in second reaction there is equal number of molecules on both sides so equilibrium is not shifted.

Conclusion

Equilibrium shifts to the reactants side by changing the volume of the system in first reaction and there is no shifting in equilibrium state for the second reaction.