The shift in the direction of the reactions at the given conditions has to be explained. Concept introduction: Le Chatelier’s principle: When a system at equilibrium is disturbed by changing the volume, pressure, temperature, concentrations of the products and concentration of the reactants, the system will adjust itself to nullify the effect and maintain the equilibrium. When concentrations of the products are increased, equilibrium will shift towards the left, producing more reactants. When concentrations of the reactants are increased, equilibrium will shift towards the left, producing more products. Increase in pressure (or decrease in volume) will shift the equilibrium to direction where there is a decrease in gaseous molecule. Decrease in pressure (or increase in volume) will shift the equilibrium towards the direction where there is an increase in the gaseous molecule. For an endothermic reaction increase in temperature will increase the rate of the forward reaction. For an exothermic reaction increase in temperature will increase the rate of the reverse reaction.

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Chapter 14.7, Problem 14.12E

(a)

Interpretation Introduction

Interpretation:

The shift in the direction of the reactions at the given conditions has to be explained.

Concept introduction:

Le Chatelier’s principle: When a system at equilibrium is disturbed by changing the volume, pressure, temperature, concentrations of the products and concentration of the reactants, the system will adjust itself to nullify the effect and maintain the equilibrium.

When concentrations of the products are increased, equilibrium will shift towards the left, producing more reactants.

When concentrations of the reactants are increased, equilibrium will shift towards the left, producing more products.

Increase in pressure (or decrease in volume) will shift the equilibrium to direction where there is a decrease in gaseous molecule. Decrease in pressure (or increase in volume) will shift the equilibrium towards the direction where there is an increase in the gaseous molecule.

For an endothermic reaction increase in temperature will increase the rate of the forward reaction. For an exothermic reaction increase in temperature will increase the rate of the reverse reaction.

(b)

Interpretation Introduction

Interpretation:

The shift in the direction of the reactions at the given conditions has to be explained.

Concept introduction:

Le Chatelier’s principle: When a system at equilibrium is disturbed by changing the volume, pressure, temperature, concentrations of the products and concentration of the reactants, the system will adjust itself to nullify the effect and maintain the equilibrium.

When concentrations of the products are increased, equilibrium will shift towards the left, producing more reactants.

When concentrations of the reactants are increased, equilibrium will shift towards the left, producing more products.

Increase in pressure (or decrease in volume) will shift the equilibrium to direction where there is a decrease in gaseous molecule. Decrease in pressure (or increase in volume) will shift the equilibrium towards the direction where there is an increase in the gaseous molecule.

For an endothermic reaction increase in temperature will increase the rate of the forward reaction. For an exothermic reaction increase in temperature will increase the rate of the reverse reaction.

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