Chapter 16, Problem 23E

Interpretation Introduction

(a)

Interpretation:

The direction of the equilibrium on increasing concentration of methane is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On increasing the concentration of methane, equilibrium shifts to the right.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

On increasing the concentration of methane, the equilibrium shifts to the right. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on increasing the concentration of methane, the equilibrium shifts to the right to decrease the concentration of methane.

Conclusion

The effect of increasing concentration of methane has been stated above.

Interpretation Introduction

(b)

Interpretation:

The effect of decreasing concentration of water is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

The equilibrium shifts to the left on decreasing concentration of water.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

On decreasing the concentration of water, the equilibrium shifts to the left. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on decreasing the concentration of water, the equilibrium shifts to the left to increase the concentration of water.

Conclusion

The effect of decreasing concentration of water has been stated above.

Interpretation Introduction

(c)

Interpretation:

The direction of the equilibrium on increasing concentration of carbonyl is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On increasing the concentration of carbonyl the equilibrium shifts to the left.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

On increasing the concentration of carbonyl, the equilibrium shifts to the left. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on increasing the concentration of carbonyl, the equilibrium shifts to the left to decrease the concentration of carbonyl.

Conclusion

The effect of increasing concentration of carbonyl has been stated above.

Interpretation Introduction

(d)

Interpretation:

The direction of the equilibrium on decreasing concentration of hydrogen gas is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On decreasing the concentration of hydrogen gas, equilibrium shifts to the right

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

On decreasing the concentration of hydrogen gas, the equilibrium shifts to the right. As according to Le Chatelier’s principle, the equilibrium alters its direction in order to counteract the change. Therefore, on decreasing the concentration of hydrogen gas, the equilibrium shifts to the right to increase the concentration of hydrogen gas.

Conclusion

The effect of decreasing concentration of hydrogen gas has been stated above.

Interpretation Introduction

(e)

Interpretation:

The direction of the equilibrium on increasing temperature is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On increasing temperature, the equilibrium shifts towards the right.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

In an endothermic reaction, as heat is being absorbed by the reactant molecules, an increase in temperature causes the equilibrium to shift towards right. Therefore, in the above reaction on increasing the temperature the equilibrium shifts towards the right.

Conclusion

The effect of increasing temperature has been stated above.

Interpretation Introduction

(f)

Interpretation:

The direction of the equilibrium decreasing temperature is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On decreasing the temperature the equilibrium shifts to the left.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

In an endothermic reaction, as heat is being absorbed by the reactant molecules, a decrease in temperature causes the equilibrium to shift towards left. Therefore, in the above reaction on increasing the temperature the equilibrium shifts towards the left.

Conclusion

The effect of decreasing temperature has been stated above.

Interpretation Introduction

(g)

Interpretation:

The direction of equilibrium on increasing volume is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On increasing the volume equilibrium shifts towards the right.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

On increasing volume, the pressure of the container decreases. Therefore, the equilibrium shifts towards the side with more number of gaseous molecules. The equilibrium shifts towards the right.

Conclusion

The effect of increasing volume has been stated above.

Interpretation Introduction

(h)

Interpretation:

The direction of the equilibrium decreasing volume is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On decreasing the volume, the equilibirum shifts towards the left.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

On decreasing volume, the pressure of the container increases so the equilibrium shifts towards the side with less number of gaseous molecules. Therefore, the equilibrium shifts towards the left.

Conclusion

The effect decreasing volume has been stated above.

Interpretation Introduction

(i)

Interpretation:

The direction of the equilibrium on adding zinc dust is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

There is no change in the equilibrium on adding zinc dust.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

In the above reaction, zinc dust has no effect on the equilibrium as it has no role in the reaction.

Conclusion

The effect of adding zinc dust has been stated above.

Interpretation Introduction

(j)

Interpretation:

The direction of the equilibrium on neon gas is to be stated for the following reaction.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Concept introduction:

Equilibrium is the state where the concentration of the reactant is equal to the concentration of the product. According to Le Chatelier’s principle, when a change is applied to a reaction, it moves in the direction in such a way to counteract the change. The changes applied may be changed in concentration, pressure, volume, and temperature.

Answer to Problem 23E

On adding xenon gas, there is no change in the equilibrium of the reaction.

Explanation of Solution

The given reaction is shown below.

${\text{CH}}_{\text{4}}\left(g\right)+{\text{H}}_{\text{2}}\text{O}\left(g\right)+heat\rightleftarrows \text{CO}\left(g\right)+3{\text{H}}_{\text{2}}\left(g\right)$

Xenon gas is an inert gas and will not react with any of the above reactant or product. Therefore, there is no effect on the equilibrium.

Conclusion

The effect of adding xenon gas has been stated above.