Chapter 6, Problem 62E

a)

Interpretation Introduction

Interpretation: Effect of reaction mixture at equilibrium as ${\text{H}}_{\text{2}}\text{O}\left(g\right)$ is removed from below reaction is to be determined.

  ${\text{CH}}_4\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)\underset{750°\text{C}}{\overset{\text{Ni cat}}{\rightleftharpoons }}\text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction: In accordance to Le Chatelier’s principle, change in reaction condition brings changes in position of equilibrium and shifts equilibrium in that direction that tends to decrease the change. It states that on addition of reactant or product in a reaction, shifts the equilibrium in the direction of decreasing the added amount. Whereas on removal of reactant or product in reaction, shifts the equilibrium in the direction of increasing the amount removed.

b)

Interpretation Introduction

Interpretation: Effect of reaction mixture at equilibrium as temperature of endothermic reaction is increased in below reaction is to be determined.

  ${\text{CH}}_4\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)\underset{750°\text{C}}{\overset{\text{Ni cat}}{\rightleftharpoons }}\text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction: In accordance to Le Chatelier’s principle change in reaction condition brings changes in position of equilibrium and shifts equilibrium in that direction that tends to decrease the change. It states that for an endothermic reaction increase in temperature tends to shift equilibrium in forward direction and for exothermic reaction it shifts in backward direction.

c)

Interpretation Introduction

Interpretation: Effect of reaction mixture at equilibrium as pressure inert gas is added in below reaction is to be determined.

  ${\text{CH}}_4\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)\underset{750°\text{C}}{\overset{\text{Ni cat}}{\rightleftharpoons }}\text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction: In accordance to Le Chatelier’s principle change in reaction condition brings changes in position of equilibrium and shifts equilibrium in that direction that tends to decrease the change. It states that with increase in pressure of container its volume decreases. Increase in volume shifts equilibrium in that direction that increases the overall volume. Decrease in volumes shifts equilibrium in that direction that has less number of moles.

d)

Interpretation Introduction

Effect of reaction mixture at equilibrium as $\text{CO}\left(g\right)$ is removed from below reaction is to be determined.

  ${\text{CH}}_4\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)\underset{750°\text{C}}{\overset{\text{Ni cat}}{\rightleftharpoons }}\text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction: In accordance to Le Chatelier’s principle, change in reaction condition brings changes in position of equilibrium and shifts equilibrium in that direction that tends to decrease the change. It states that on addition of reactant or product in a reaction, shifts the equilibrium in the direction of decreasing the added amount. Whereas on removal of reactant or product in reaction, shifts the equilibrium in the direction of increasing the amount removed.

e)

Interpretation Introduction

Interpretation: Effect of reaction mixture at equilibrium as volume is tripled in below reaction is to be determined.

  ${\text{CH}}_4\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)\underset{750°\text{C}}{\overset{\text{Ni cat}}{\rightleftharpoons }}\text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction: In accordance to Le Chatelier’s principle change in reaction condition brings changes in position of equilibrium and shifts equilibrium in that direction that tends to decrease the change. It states that with increase in pressure of container its volume decreases. Increase in volume shifts equilibrium in that direction that increases the overall volume. Decrease in volumes shifts equilibrium in that direction that has less number of moles.