Chapter 19, Problem 138A

Interpretation Introduction

Interpretation : The position of equilibrium changes on increasing the pressure to be explained.

Concept Introduction : The equilibrium law, commonly known as Le Chatelier's principles, is used to forecast how certain changes will affect a system in chemical equilibrium (that is the change in pressure or temperature).

Answer to Problem 138A

The position of equilibrium changes to the right side on increasing the pressure.

Explanation of Solution

The reaction is given as

  ${\text{2H}}_{\text{2}}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{H}}_{\text{2}}\text{O}\left(g\right)+\text{heat}$

By increasing the pressure, the equilibrium of the reaction shifts to the right side of the reaction.

Interpretation Introduction

Interpretation : The position of equilibrium changes on adding a catalyst to be explained.

Concept Introduction : The equilibrium law, commonly known as Le Chatelier's principles, is used to forecast how certain changes will affect a system in chemical equilibrium (that is the change in pressure or temperature).

Answer to Problem 138A

The position of equilibrium remains unchanged on addition of a catalyst.

Explanation of Solution

The reaction is given as

  ${\text{2H}}_{\text{2}}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{H}}_{\text{2}}\text{O}\left(g\right)+\text{heat}$

The addition of a catalyst influences the rate of the reaction but does not influence the position of equilibrium.

The position of equilibrium does not change with the addition of a catalyst.

Interpretation Introduction

Interpretation : The position of equilibrium changes on increasing the concentration of hydrogen to be explained.

Concept Introduction : The equilibrium law, commonly known as Le Chatelier's principles, is used to forecast how certain changes will affect a system in chemical equilibrium (that is the change in pressure or temperature).

Answer to Problem 138A

The position of equilibrium changes to the right side on increasing the concentration of hydrogen.

Explanation of Solution

The reaction is given as

  ${\text{2H}}_{\text{2}}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{H}}_{\text{2}}\text{O}\left(g\right)+\text{heat}$

By increasing the concentration of hydrogen gas, the equilibrium of the reaction shifts to the right side of the reaction.

Interpretation Introduction

Interpretation : The position of equilibrium changes on cooling the reaction mixture to be explained.

Concept Introduction : The equilibrium law, commonly known as Le Chatelier's principles, is used to forecast how certain changes will affect a system in chemical equilibrium (that is the change in pressure or temperature).

Answer to Problem 138A

The position of equilibrium changes to the right side on cooling the reaction mixture.

Explanation of Solution

The reaction is given as

  ${\text{2H}}_{\text{2}}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{H}}_{\text{2}}\text{O}\left(g\right)+\text{heat}$

By cooling the reaction mixture, the equilibrium of the reaction shifts to the right side of reaction.

Interpretation Introduction

Interpretation : The position of equilibrium changes on removing water vapor from the container to be explained.

Concept Introduction : The equilibrium law, commonly known as Le Chatelier's principles, is used to forecast how certain changes will affect a system in chemical equilibrium (that is the change in pressure or temperature).

Answer to Problem 138A

The position of equilibrium changes to the right side on removing water vapor from the container.

Explanation of Solution

The reaction is given as

  ${\text{2H}}_{\text{2}}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons 2{\text{H}}_{\text{2}}\text{O}\left(g\right)+\text{heat}$

On removing the water vapor from the container, the equilibrium of the reaction shifts to the right side of the reaction.