The reason for the shift in the direction of the reaction 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, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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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Answer 2

Question

Chapter 14, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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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Answer 3

Question

Chapter 14, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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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Answer 4

Question

Chapter 14, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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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Answer 5

Chapter 14, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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.

Answer 6

Chapter 14, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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.

Answer 7

Chapter 14, Problem 14.22QP

Interpretation Introduction

Interpretation:

The reason for the shift in the direction of the reaction 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.

Answer 8

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Answer 11

Ch. 14.1 - Synthesis gas (a mixture of CO and H2) is...Ch. 14.1 - Two substances A and B react to produce substance...Ch. 14.2 - a. Write the equilibrium-constant expression Kc...Ch. 14.2 - When 1.00 mol each of carbon monoxide and water...Ch. 14.2 - Hydrogen sulfide, a colorless gas with a foul...Ch. 14.2 - Phosphorus pentachloride dissociates on heating:...Ch. 14.2 - Consider the following hypothetical reactions. The...Ch. 14.3 - The Mond process for purifying nickel involves the...Ch. 14.4 - The equilibrium constant Kc for the reaction...Ch. 14.5 - A 10.0-L vessel contains 0.0015 mol CO2 and 0.10...

Solution Summary: The author explains Le Chatelier's principle that when a system at equilibrium is disturbed, it will adjust itself to nullify the effect and maintain the equilibrium.

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