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Chapter 13: Problem 68

Hydrogen for use in ammonia production is produced by the reaction $$ \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \stackrel{\mathrm{Nicatalyst}}{750^{\circ} \mathrm{C}} \mathrm{CO}(g)+3 \mathrm{H}_{2}(g) $$ What will happen to a reaction mixture at equilibrium if a. \(\mathrm{H}_{2} \mathrm{O}(g)\) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert gas is added to a rigid reaction container? d. \(\mathrm{CO}(g)\) is removed? e. the volume of the container is tripled?

Short Answer

Expert verified
a. If \(H_2O(g)\) is removed, the reaction will shift to the left, increasing concentrations of \(CH_4(g)\) and \(H_2O(g)\), and decreasing concentrations of \(CO(g)\) and \(H_2(g)\). b. If the temperature is increased, the reaction will shift to the right, increasing concentrations of \(CO(g)\) and \(H_2(g)\) and decreasing concentrations of \(CH_4(g)\) and \(H_2O(g)\). c. If an inert gas is added, there will be no change to the equilibrium position or the concentrations of the reacting species. d. If \(CO(g)\) is removed, the reaction will shift to the right, decreasing concentrations of \(CH_4(g)\) and \(H_2O(g)\), and increasing concentrations of \(CO(g)\) and \(H_2(g)\). e. If the volume of the container is tripled, the reaction will shift to the right, increasing concentrations of \(CO(g)\) and \(H_2(g)\), and decreasing concentrations of \(CH_4(g)\) and \(H_2O(g)\).

Step by step solution

01

Scenario A: Removal of \(H_2O(g)\)

When \(H_2O(g)\) is removed from the reaction mixture, the concentration of \(H_2O(g)\) decreases. According to Le Chatelier's principle, the system will adjust its equilibrium position to counteract the disturbance. In this case, the reaction will shift to the left to produce more \(H_2O(g)\) and consume \(CO(g)\) and \(H_2(g)\). Therefore, the concentration of \(CH_4(g)\) and \(H_2O(g)\) will increase, while the concentration of \(CO(g)\) and \(H_2(g)\) will decrease.
02

Scenario B: Increase in temperature (endothermic reaction)

As the reaction is endothermic, increasing the temperature will cause the system to absorb more heat. According to Le Chatelier's principle, the system will adjust its equilibrium position to counteract the disturbance. In this case, the reaction will shift to the right as this is the direction of the endothermic reaction. The equilibrium concentrations of \(CO(g)\) and \(H_2(g)\) will increase, while the equilibrium concentrations of \(CH_4(g)\) and \(H_2O(g)\) will decrease.
03

Scenario C: Addition of an inert gas to a rigid reaction container

When an inert gas is added to a rigid reaction container, the total pressure of the system increases, but the partial pressures of the reacting species remain unchanged. The inert gas does not participate in the reaction and, therefore, does not affect the equilibrium. In this case, there will be no change to the equilibrium position or the concentrations of the reacting species.
04

Scenario D: Removal of \(CO(g)\)

When \(CO(g)\) is removed from the reaction mixture, the concentration of \(CO(g)\) decreases. According to Le Chatelier's principle, the system will adjust its equilibrium position to counteract the disturbance. In this case, the reaction will shift to the right to produce more \(CO(g)\) and consume \(CH_4(g)\) and \(H_2O(g)\). Therefore, the concentration of \(CH_4(g)\) and \(H_2O(g)\) will decrease, while the concentration of \(CO(g)\) and \(H_2(g)\) will increase.
05

Scenario E: Tripling the volume of the container

When the volume of the container is tripled, the pressure of the system decreases. According to Le Chatelier's principle, the system will adjust its equilibrium position to counteract the disturbance. As the forward reaction produces more moles of gas (4 moles) than the reverse reaction (2 moles), the system will shift to the side where there is a greater number of moles to restore pressure. In this case, the reaction will shift to the right. The equilibrium concentrations of \(CO(g)\) and \(H_2(g)\) will increase, while the equilibrium concentrations of \(CH_4(g)\) and \(H_2O(g)\) will decrease.

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Most popular questions from this chapter

At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide: $$ \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) $$ Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations are found to be \(\left[\mathrm{N}_{2}\right]=\) \(0.041 \mathrm{M},\left[\mathrm{O}_{2}\right]=0.0078 M\), and \([\mathrm{NO}]=4.7 \times 10^{-4} M .\) Calcu- late the value of \(K\) for the reaction.

A sample of \(S_{8}(g)\) is placed in an otherwise empty rigid container at \(1325 \mathrm{~K}\) at an initial pressure of \(1.00 \mathrm{~atm}\), where it decomposes to \(\mathrm{S}_{2}(g)\) by the reaction $$ \mathrm{S}_{8}(g) \rightleftharpoons 4 \mathrm{~S}_{2}(g) $$ At equilibrium, the partial pressure of \(\mathrm{S}_{\mathrm{g}}\) is \(0.25 \mathrm{~atm} .\) Calculate \(K\). for this reaction at \(1325 \mathrm{~K}\).

Consider the following reaction: $$ \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CO}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g) $$ Amounts of \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CO}, \mathrm{H}_{2}\), and \(\mathrm{CO}_{2}\) are put into \(\underline{\mathrm{a}}\) flask so that the composition corresponds to an equilibrium position. If the CO placed in the flask is labeled with radioactive \({ }^{14} \mathrm{C}\), will \({ }^{14} \mathrm{C}\) be found only in CO molecules for an indefinite period of time? Explain.

At \(25^{\circ} \mathrm{C}, K_{\mathrm{p}}=5.3 \times 10^{5}\) for the reaction $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$ When a certain partial pressure of \(\mathrm{NH}_{3}(g)\) is put into an otherwise empty rigid vessel at \(25^{\circ} \mathrm{C}\), equilibrium is reached when \(50.0 \%\) of the original ammonia has decomposed. What was the original partial pressure of ammonia before any decomposition occurred?

The gas arsine, \(\mathrm{AsH}_{3}\), decomposes as follows: $$ 2 \mathrm{AsH}_{3}(g) \rightleftharpoons 2 \mathrm{As}(s)+3 \mathrm{H}_{2}(g) $$ In an experiment at a certain temperature, pure \(\operatorname{AsH}_{3}(g)\) was placed in an empty, rigid, sealed flask at a pressure of \(392.0\) torr. After 48 hours the pressure in the flask was observed to be constant at \(488.0\) torr. a. Calculate the equilibrium pressure of \(\mathrm{H}_{2}(\mathrm{~g})\). b. Calculate \(K_{\mathrm{p}}\) for this reaction.
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