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13.84 For the water-gas shift reaction CO(g) + H2O(g) = CO2(g) + H2(g), AH° = in an equilibrium mixture increase or decrease when the temperature is increased? How does K. change when the temperature is decreased? Justify your answers using Le Châtelier's principle. -41.2 kJ, does the amount of H2

13.84 For the water-gas shift reaction CO(g) + H2O(g) = CO2(g) + H2(g), AH° = in an equilibrium mixture increase or decrease when the temperature is increased? How does K. change when the temperature is decreased? Justify your answers using Le Châtelier's principle. -41.2 kJ, does the amount of H2

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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# Le Châtelier's Principle (Sections 13.6–13.10) ## 13.80 Consider the following equilibrium: \( \text{Ag}^+(aq) + \text{Cl}^-(aq) \rightleftharpoons \text{AgCl}(s) \). Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (a) Adding NaCl (b) Adding AgNO\(_3\) (c) Adding NH\(_3\), which reacts with Ag\(^+\) to form the complex ion \( \text{Ag(NH}_3\text{)}_2^+ \) (d) Removing Cl\(^-\); also account for the change using the reaction quotient Q\(_c\). ## 13.81 Will the concentration of NO\(_2\) increase, decrease, or remain the same when the equilibrium \( \text{NOCl}(g) + \text{NO}_2(g) \rightleftharpoons \text{NOCl}(g) + \text{NO}_2(g) \) is disturbed by the following changes? (a) Adding NOCl (b) Adding NO (c) Removing NO (d) Adding NO\(_2\)Cl; also account for the change using the reaction quotient Q\(_c\). ## 13.82 When each of the following equilibria is disturbed by increasing the pressure as a result of decreasing the volume, does the number of moles of reaction products increase, decrease, or remain the same? (a) \( 2\text{CO}(g) \rightleftharpoons 2\text{CO}(g) + \text{O}_2(g) \) (b) \( \text{N}_2(g) + 2\text{Cl}_2(g) \rightleftharpoons 2\text{NOCl}(g) \) (c) \( \text{Si}(s) + 2\text{Cl}_2(g) \rightleftharpoons \text{SiCl}_4(g) \) ## 13.83 For each of the following equilibria, use Le Châtelier's principle to predict the direction of reaction when the volume is increased. (a) \( \text{C}(s) + \text
Transcribed Image Text:# Le Châtelier's Principle (Sections 13.6–13.10) ## 13.80 Consider the following equilibrium: \( \text{Ag}^+(aq) + \text{Cl}^-(aq) \rightleftharpoons \text{AgCl}(s) \). Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (a) Adding NaCl (b) Adding AgNO\(_3\) (c) Adding NH\(_3\), which reacts with Ag\(^+\) to form the complex ion \( \text{Ag(NH}_3\text{)}_2^+ \) (d) Removing Cl\(^-\); also account for the change using the reaction quotient Q\(_c\). ## 13.81 Will the concentration of NO\(_2\) increase, decrease, or remain the same when the equilibrium \( \text{NOCl}(g) + \text{NO}_2(g) \rightleftharpoons \text{NOCl}(g) + \text{NO}_2(g) \) is disturbed by the following changes? (a) Adding NOCl (b) Adding NO (c) Removing NO (d) Adding NO\(_2\)Cl; also account for the change using the reaction quotient Q\(_c\). ## 13.82 When each of the following equilibria is disturbed by increasing the pressure as a result of decreasing the volume, does the number of moles of reaction products increase, decrease, or remain the same? (a) \( 2\text{CO}(g) \rightleftharpoons 2\text{CO}(g) + \text{O}_2(g) \) (b) \( \text{N}_2(g) + 2\text{Cl}_2(g) \rightleftharpoons 2\text{NOCl}(g) \) (c) \( \text{Si}(s) + 2\text{Cl}_2(g) \rightleftharpoons \text{SiCl}_4(g) \) ## 13.83 For each of the following equilibria, use Le Châtelier's principle to predict the direction of reaction when the volume is increased. (a) \( \text{C}(s) + \text
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