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Chapter 13: Problem 78

Hydrogen for use in ammonia production is produced by the reaction $$\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \frac{\text { Nicatalyst }}{750^{\circ} \mathrm{C}} \mathrm{CO}(g)+3 \mathrm{H}_{2}(g)$$ 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
In summary: a. If H2O(g) is removed, the reaction shifts to the left (toward the reactants). b. If the temperature is increased in an endothermic reaction, the reaction shifts to the right (toward the products). c. Adding an inert gas to a rigid reaction container does not change the equilibrium position. d. If CO(g) is removed, the reaction shifts to the right (toward the products). e. If the volume of the container is tripled, the reaction shifts to the right (toward the products) to re-establish equilibrium.

Step by step solution

01

Identify the side where H2O(g) is present.

In the given reaction, H2O(g) is on the reactant side.
02

Analyze the effect of removing H2O(g) on the equilibrium position.

According to Le Chatelier's principle, when H2O(g) is removed, the reaction will shift in the direction which will increase the concentration of H2O(g). Thus, the reaction will shift to the left (toward the reactants). #b. The temperature is increased (the reaction is endothermic)#
03

Analyze the effect of increasing temperature on the equilibrium position.

As the reaction is endothermic, it means the reaction absorbs heat to proceed. According to Le Chatelier's principle, upon increasing the temperature, the reaction will shift in the direction which absorbs the added heat. Hence, the reaction will shift to the right (toward the products). #c. An inert gas is added to a rigid reaction container#
04

Analyze the effect of adding an inert gas on the equilibrium position.

In a rigid reaction container, when an inert gas is added, the overall pressure increases but the partial pressures of each component remain unchanged. Since the equilibrium position doesn't rely on the total pressure but only on the partial pressures, the addition of an inert gas in a rigid reaction container does not cause a shift in the equilibrium position. #d. CO(g) is removed#
05

Identify the side where CO(g) is present.

In the given reaction, CO(g) is on the product side.
06

Analyze the effect of removing CO(g) on the equilibrium position.

According to Le Chatelier's principle, when CO(g) is removed, the reaction will shift in the direction which will increase the concentration of CO(g). Thus, the reaction will shift to the right (toward the products). #e. The volume of the container is tripled#
07

Analyze the effect of tripling the volume on the equilibrium position.

When the volume of the container is tripled, the pressure in the system decreases. According to Le Chatelier's principle, the reaction will shift in the direction which has more moles of gas to counteract the change in pressure. Since there are 2 moles of gas on the reactant side and 4 moles of gas on the product side, the reaction will shift to the right (toward the products) to re-establish equilibrium.

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Most popular questions from this chapter

At \(2200^{\circ} \mathrm{C}, K_{\mathrm{p}}=0.050\) for the reaction $$\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$$ What is the partial pressure of NO in equilibrium with \(\mathrm{N}_{2}\) and \(\mathrm{O}_{2}\) that were placed in a flask at initial pressures of 0.80 and \(0.20 \mathrm{atm},\) respectively?

The reaction to prepare methanol from carbon monoxide and hydrogen $$\mathrm{CO}(g)+\mathrm{H}_{2}(g) \leftrightharpoons \mathrm{CH}_{3} \mathrm{OH}(g)$$ is exothermic. If you wanted to use this reaction to produce methanol commercially, would high or low temperatures favor a maximum yield? Explain.

Which of the following statements is(are) true? Correct the false statement(s). a. When a reactant is added to a system at equilibrium at a given temperature, the reaction will shift right to reestablish equilibrium. b. When a product is added to a system at equilibrium at a given temperature, the value of K for the reaction will increase when equilibrium is reestablished. c. When temperature is increased for a reaction at equilibrium, the value of K for the reaction will increase. d. When the volume of a reaction container is increased for a system at equilibrium at a given temperature, the reaction will shift left to reestablish equilibrium. e. Addition of a catalyst (a substance that increases the speed of the reaction) has no effect on the equilibrium position.

Old-fashioned "smelling salts" consist of ammonium carbonate, (NH $_{4} )_{2} \mathrm{CO}_{3}$ . The reaction for the decomposition of ammonium carbonate $$\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(s) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$$ is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?

At a particular temperature, 8.1 moles of \(\mathrm{NO}_{2}\) gas are placed in a 3.0 -L container. Over time the \(\mathrm{NO}_{2}\) decomposes to \(\mathrm{NO}\) and \(\mathrm{O}_{2} :\) $$2 \mathrm{NO}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)$$ At equilibrium the concentration of \(\mathrm{NO}(g)\) was found to be 1.4 \(\mathrm{mol} / \mathrm{L}\) . Calculate the value of \(K\) for this reaction.
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