Chapter 6.6, Problem 6.20P

Interpretation Introduction

(a)

Interpretation:

The shift of the direction is to be found to attain equilibrium for the reaction ${\text{H}}_{\text{2}}+{\text{Cl}}_{\text{2}}\underset{}{\overset{}{\rightleftarrows }}\text{2HCl}$ when there is an increase in ${\text{H}}_{\text{2}}$.

Concept Introduction:

If the number of reactants and products is not equal, then the system is said to be in a non-equilibrium state. Hence, to attain an equilibrium, it will shift to either direction to be in equilibrium.

Interpretation Introduction

(b)

Interpretation:

The shift of the direction is to be found to attain equilibrium for the reaction ${\text{H}}_{\text{2}}+{\text{Cl}}_{\text{2}}\underset{}{\overset{}{\rightleftarrows }}\text{2HCl}$ when there is an increase in $\text{HCl}$.

Concept Introduction:

If the number of reactants and products is not equal, then the system is said to be a nonequilibrium state.

Hence, to attain an equilibrium, it will shift to either direction to be in equilibrium.

Interpretation Introduction

(c)

Interpretation:

The shift of the direction is to be found to attain equilibrium for the reaction ${\text{H}}_{\text{2}}+{\text{Cl}}_{\text{2}}\underset{}{\overset{}{\rightleftarrows }}\text{2HCl}$ when there is a decrease in ${\text{Cl}}_{\text{2}}$.

Concept Introduction:

If the number of reactants and products is not equal, then the system is said to be a non-equilibrium state.

Hence, to attain an equilibrium, it will shift to either direction to be in equilibrium.

Interpretation Introduction

(d)

Interpretation:

The shift of the direction is to be found to attain equilibrium for the reaction ${\text{H}}_{\text{2}}+{\text{Cl}}_{\text{2}}\underset{}{\overset{}{\rightleftarrows }}2\text{HCl}$ when there is a decrease in $\text{HCl}$.

Concept Introduction:

If the number of reactants and products is not equal, then the system is said to be a nonequilibrium state.

Hence, to attain an equilibrium, it will shift to either direction to be in equilibrium.