Chapter 17, Problem 63A

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Interpretation Introduction

(a)

Interpretation:

The effect on the temperature of the given equilibrium by increasing the yield of ethane needs to be explained.

Concept introduction:

By changing the temperature, the equilibrium shifts to attain the initial equilibrium state.

Answer to Problem 63A

When concentration of ethane or product is increased then the equilibrium state is shifted to the left side or the reactants side to attain the equilibrium state and temperature is also increased.

Explanation of Solution

The given equilibrium reaction is

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(\text{g}\right){\text{+H}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{C}}_{\text{2}}{\text{H}}_{\text{6}}\left(\text{g}\right)\text{+Heat}$

According to Le Chatelier’s principle, when concentration of ethane or product is increased then the equilibrium state is shifted to the left side or the reactants side to attain the equilibrium state by increasing the temperaturewhich favors an exothermic reaction.

(b)

Interpretation Introduction

Interpretation:

The change in the temperature of the system due to decrease in the concentration of ethylene or reactant needs to be explained.

Concept introduction:

By changing the temperature, the equilibrium shifts to attain the initial equilibrium state.

Answer to Problem 63A

The temperature is decreased when the concentration of reactant is increased then the equilibrium is shift towards the right side with the formation of additional product.

Explanation of Solution

The given equilibrium reaction is as follows:

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(\text{g}\right){\text{+H}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{C}}_{\text{2}}{\text{H}}_{\text{6}}\left(\text{g}\right)\text{+Heat}$

The temperature is decreased when the concentration of reactants is increased then the equilibrium shifts towards the right side with the formation of additional product.

The given equilibrium reaction is as follows:

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(\text{g}\right){\text{+H}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{C}}_{\text{2}}{\text{H}}_{\text{6}}\left(\text{g}\right)\text{+Heat}$

The given reaction is an exothermic reaction. So, the equilibrium position shifts to right side by decreasing the temperature because of decreasing the concentration of ethylene.

(c)

Interpretation Introduction

Interpretation:

The effect on the temperature by increasing the concentration of hydrogen needs to be explained.

Concept introduction:

By changing the temperature, the equilibrium shifts to attain the initial equilibrium state.

Answer to Problem 63A

When concentration of hydrogen is increased then the equilibrium sifts to right side with decreasing temperature which favors exothermic reactions.

Explanation of Solution

The given equilibrium reaction is

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}\left(\text{g}\right){\text{+H}}_{\text{2}}\left(\text{g}\right)\rightleftharpoons {\text{C}}_{\text{2}}{\text{H}}_{\text{6}}\left(\text{g}\right)\text{+Heat}$

By increasing the concentration of hydrogen gas, equilibrium shifts to right side with deceasing temperature which favors the exothermic reaction and due to addition of hydrogen concentration additional products are formed.