Chapter 16, Problem 24E

Interpretation Introduction

(a)

Interpretation:

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

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

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

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

On increasing the concentration of ethylene, 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 ethylene, the equilibrium shifts to the right to decrease the concentration of ethylene.

Conclusion

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

Interpretation Introduction

(b)

Interpretation:

The effect of decreasing concentration of ${\text{O}}_3$ is to be stated for the following reaction.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

The equilibrium shifts to the left on decreasing concentration of ${\text{O}}_3$.

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

On decreasing the concentration of ${\text{O}}_3$, 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 ${\text{O}}_3$, the equilibrium shifts to the left to increase the concentration of ${\text{O}}_3$.

Conclusion

The effect of decreasing concentration of ${\text{O}}_3$ has been stated above.

Interpretation Introduction

(c)

Interpretation:

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

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

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

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

On increasing the concentration of formaldehyde, 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 formaldehyde, the equilibrium shifts to the left to decrease the concentration of formaldehyde.

Conclusion

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

Interpretation Introduction

(d)

Interpretation:

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

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

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

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

On decreasing the concentration of oxygen 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 oxygen gas, the equilibrium shifts to the right to increase the concentration of oxygen gas.

Conclusion

The effect of decreasing concentration of oxygen 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.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

On increasing temperature, the equilibrium shifts towards the left.

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

It is an exothermic reaction as heat is released. In an exothermic reaction, as heat is being released with the products, an increase in temperature causes the equilibrium to shift towards left and consumes more heat energy for the formation of reactant. Therefore, in the above reaction on increasing the temperature the equilibrium shifts towards the left.

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.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

On decreasing the temperature the equilibrium shifts to the right.

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

It is an exothermic reaction as heat is released. In an exothermic reaction, as heat is being released with the products, a decrease in temperature causes the equilibrium to shift towards right. Therefore, in the above reaction on decreasing the temperature the equilibrium shifts towards the right.

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.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

On increasing the volume equilibrium shifts towards the right.

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

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

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 neon inert gas is to be stated for the following reaction.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

There is no change in the equilibrium on adding neon inert gas.

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

Neon is an inert gas. It does not participate in this reaction. Therefore, in the above reaction, neon inert gas has no effect on the equilibrium as it has no role in the reaction.

Conclusion

The effect of adding neon inert gas has been stated above.

Interpretation Introduction

(j)

Interpretation:

The direction of the equilibrium in the presence of ultraviolet light is to be stated for the following reaction.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

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 24E

In the presence of ultraviolet light, there is no change in the equilibrium of the reaction.

Explanation of Solution

The given reaction is shown below.

${\text{2C}}_2{\text{H}}_4\left(g\right)+2{\text{O}}_3\left(g\right)\rightleftarrows 4{\text{CH}}_{\text{2}}\text{O}\left(g\right)+{\text{O}}_{\text{2}}\left(g\right)+heat$

The abiovbe reaction does not affected by exposing ultaviolet light. Therefore, there is no effect on the equilibrium.

Conclusion

The effect of ultraviolet light has been stated above.