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Chapter 13: Problem 65

An important reaction in the commercial production of hydrogen is $$ \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(g) $$ How will this system at equilibrium shift in each of the five following cases? a. Gaseous carbon dioxide is removed. b. Water vapor is added. c. In a rigid reaction container, the pressure is increased by adding helium gas. d. The temperature is increased (the reaction is exothermic). e. The pressure is increased by decreasing the volume of the reaction container.

Short Answer

Expert verified
a. The system will shift to the right, favoring the formation of hydrogen and carbon dioxide. b. The system will shift to the right, favoring the formation of hydrogen and carbon dioxide. c. There will be no shift in the reaction equilibrium. d. The system will shift to the left, favoring the formation of carbon monoxide and water vapor. e. There will be no shift in the reaction equilibrium.

Step by step solution

01

Identify affected component and direction

Gaseous carbon dioxide (CO₂) is a product of the reaction. Since it is removed, its concentration will decrease.
02

Apply Le Chatelier's principle

To counteract the decrease in CO₂ concentration, the system will shift the equilibrium to the right (production of more CO₂). Thus, the reaction will favor the formation of hydrogen and carbon dioxide. #b. Water vapor is added.#
03

Identify affected component and direction

Water vapor (H₂O) is a reactant in the reaction. Since it is added, its concentration will increase.
04

Apply Le Chatelier's principle

To counteract the increase in H₂O concentration, the system will shift the equilibrium to the right. Thus, the reaction will favor the formation of hydrogen and carbon dioxide. #c. In a rigid reaction container, the pressure is increased by adding helium gas.#
05

Identify affected component and direction

The pressure is increased by adding helium gas (an inert gas). This change does not directly affect the concentrations of the reactants or products in the reaction.
06

Apply Le Chatelier's principle

Since there is no change in the concentrations of the components, the system's equilibrium position will not be affected. Therefore, there will be no shift in the reaction equilibrium. #d. The temperature is increased (the reaction is exothermic).#
07

Identify affected component and direction

The temperature of the system is increased. Since the reaction is exothermic, heat can be considered as a product.
08

Apply Le Chatelier's principle

To counteract the increase in temperature, the system will shift the equilibrium to the left (consume more heat). Thus, the reaction will favor the formation of carbon monoxide and water vapor. #e. The pressure is increased by decreasing the volume of the reaction container.#
09

Identify affected component and direction

The pressure is increased by decreasing the volume of the reaction container. This change will affect the concentrations of the reactants and products equally.
10

Determine the shift direction based on the number of moles of gas

Since the number of moles of gas on the left side (CO + H₂O) is equal to the number of moles on the right side (H₂ + CO₂), the reaction's equilibrium position will not shift in response to the pressure change. Thus, there will be no shift in the reaction equilibrium.

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Most popular questions from this chapter

The equilibrium constant \(K_{\mathrm{p}}\) for the reaction $$ \mathrm{CCl}_{4}(g) \rightleftharpoons \mathrm{C}(s)+2 \mathrm{Cl}_{2}(g) $$ at \(700^{\circ} \mathrm{C}\) is \(0.76 .\) Detemine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of \(1.20 \mathrm{~atm}\) at \(700^{\circ} \mathrm{C}\).

Given \(K=3.50\) at \(45^{\circ} \mathrm{C}\) for the reaction $$ \mathrm{A}(g)+\mathrm{B}(g) \rightleftharpoons \mathrm{C}(g) $$ and \(K=7.10\) at \(45^{\circ} \mathrm{C}\) for the reaction $$ 2 \mathrm{~A}(g)+\mathrm{D}(g) \rightleftharpoons \mathrm{C}(g) $$ what is the value of \(K\) at the same temperature for the reaction $$ \mathrm{C}(g)+\mathrm{D}(g) \rightleftharpoons 2 \mathrm{~B}(g) $$ What is the value of \(K_{\mathrm{p}}\) at \(45^{\circ} \mathrm{C}\) for the reaction? Starting with \(1.50\) atm partial pressures of both \(\mathrm{C}\) and \(\mathrm{D}\), what is the mole fraction of \(\mathrm{B}\) once equilibrium is reached?

For the reaction \(\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g), K_{\mathrm{p}}=0.25\) at a cer- tain temperature. If \(0.040\) atm of \(\mathrm{N}_{2} \mathrm{O}_{4}\) is reacted initially, calculate the equilibrium partial pressures of \(\mathrm{NO}_{2}(g)\) and \(\mathrm{N}_{2} \mathrm{O}_{4}(g)\).

Lexan is a plastic used to make compact discs, eyeglass lenses, and bullet- proof glass. One of the compounds used to make Lexan is phosgene \(\left(\mathrm{COCl}_{2}\right)\), an extremely poisonous gas. Phosgene decomposes by the reaction $$ \mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g) $$ for which \(K_{\mathrm{p}}=6.8 \times 10^{-9}\) at \(100^{\circ} \mathrm{C}\). If pure phosgene at an jnitial pressure of \(1.0\) atm decomposes, calculate the equilibrium pressures of all species.

The value of the equilibrium constant \(K\) depends on which of the following (more than one answer may be correct)? a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.
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