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Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = 10.4 kJ, and Ke = 1.80 x 10-2, at 698 K: 2HI(g) H₂(g) + 1₂ (9) If the temperature on the equilibrium system is suddenly increased: The value of Ke Oincreases decreases Oremains the same The value of Q Ols less than Ke Ols greater than Ke Ols equal to Ke S The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of I2 will Oincrease Odecrease Oremain the same

Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = 10.4 kJ, and Ke = 1.80 x 10-2, at 698 K: 2HI(g) H₂(g) + 1₂ (9) If the temperature on the equilibrium system is suddenly increased: The value of Ke Oincreases decreases Oremains the same The value of Q Ols less than Ke Ols greater than Ke Ols equal to Ke S The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of I2 will Oincrease Odecrease Oremain the same

Chemistry
Chemistry
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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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Equilibrium and Temperature Changes **Chemical Equilibrium Reaction:** Consider the following system at equilibrium where: - Change in enthalpy (\( \Delta H^\circ \)) = 10.4 kJ - Equilibrium constant (\( K_c \)) = \( 1.80 \times 10^{-2} \) - Temperature = 698 K \[ 2 \text{HI}(g) \rightleftharpoons \text{H}_2(g) + \text{I}_2(g) \] **Scenario:** If the temperature on the equilibrium system is suddenly increased: 1. **The value of \( K_c \):** - Increases - Decreases - Remains the same 2. **The value of \( Q_c \):** - Is less than \( K_c \) - Is greater than \( K_c \) - Is equal to \( K_c \) 3. **The reaction must:** - Run in the forward direction to reestablish equilibrium - Run in the reverse direction to reestablish equilibrium - Remain in the current position, since it is already at equilibrium 4. **The concentration of \( I_2 \) will:** - Increase - Decrease - Remain the same This setup explores how temperature changes can affect the position of equilibrium, the equilibrium constant, and the reaction quotient, offering insights into Le Chatelier's principle and endothermic reactions.
Transcribed Image Text:### Equilibrium and Temperature Changes **Chemical Equilibrium Reaction:** Consider the following system at equilibrium where: - Change in enthalpy (\( \Delta H^\circ \)) = 10.4 kJ - Equilibrium constant (\( K_c \)) = \( 1.80 \times 10^{-2} \) - Temperature = 698 K \[ 2 \text{HI}(g) \rightleftharpoons \text{H}_2(g) + \text{I}_2(g) \] **Scenario:** If the temperature on the equilibrium system is suddenly increased: 1. **The value of \( K_c \):** - Increases - Decreases - Remains the same 2. **The value of \( Q_c \):** - Is less than \( K_c \) - Is greater than \( K_c \) - Is equal to \( K_c \) 3. **The reaction must:** - Run in the forward direction to reestablish equilibrium - Run in the reverse direction to reestablish equilibrium - Remain in the current position, since it is already at equilibrium 4. **The concentration of \( I_2 \) will:** - Increase - Decrease - Remain the same This setup explores how temperature changes can affect the position of equilibrium, the equilibrium constant, and the reaction quotient, offering insights into Le Chatelier's principle and endothermic reactions.
### Understanding Equilibrium Changes with Temperature **System at Equilibrium:** - **Reaction:** \(\text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g)\) - **Standard Enthalpy Change (\(\Delta H^\circ\)):** 108 kJ - **Equilibrium Constant (\(K_c\)):** 1.29 x 10\(^{-2}\), at 600 K #### Effects of a Temperature Increase: **The value of \(K_c\):** - \(\circ\) Increases - \(\circ\) Decreases - \(\circ\) Remains the same **The value of \(Q_c\):** - \(\circ\) Is less than \(K_c\) - \(\circ\) Is greater than \(K_c\) - \(\circ\) Is equal to \(K_c\) **Reaction Direction:** - \(\circ\) Run in the forward direction to reestablish equilibrium - \(\circ\) Run in the reverse direction to reestablish equilibrium - \(\circ\) Remain in the current position, since it is already at equilibrium **The concentration of \(Cl_2\) will:** - \(\circ\) Increase - \(\circ\) Decrease - \(\circ\) Remain the same ### Discussion: When considering changes in temperature and their effect on equilibrium, it's essential to apply Le Chatelier's Principle. Since the reaction is endothermic (\(\Delta H^\circ\) is positive), an increase in temperature will favor the forward reaction, leading to an increase in \(K_c\). ### Graphs/Diagrams Explanation: - There are no graphs or diagrams in this image.
Transcribed Image Text:### Understanding Equilibrium Changes with Temperature **System at Equilibrium:** - **Reaction:** \(\text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g)\) - **Standard Enthalpy Change (\(\Delta H^\circ\)):** 108 kJ - **Equilibrium Constant (\(K_c\)):** 1.29 x 10\(^{-2}\), at 600 K #### Effects of a Temperature Increase: **The value of \(K_c\):** - \(\circ\) Increases - \(\circ\) Decreases - \(\circ\) Remains the same **The value of \(Q_c\):** - \(\circ\) Is less than \(K_c\) - \(\circ\) Is greater than \(K_c\) - \(\circ\) Is equal to \(K_c\) **Reaction Direction:** - \(\circ\) Run in the forward direction to reestablish equilibrium - \(\circ\) Run in the reverse direction to reestablish equilibrium - \(\circ\) Remain in the current position, since it is already at equilibrium **The concentration of \(Cl_2\) will:** - \(\circ\) Increase - \(\circ\) Decrease - \(\circ\) Remain the same ### Discussion: When considering changes in temperature and their effect on equilibrium, it's essential to apply Le Chatelier's Principle. Since the reaction is endothermic (\(\Delta H^\circ\) is positive), an increase in temperature will favor the forward reaction, leading to an increase in \(K_c\). ### Graphs/Diagrams Explanation: - There are no graphs or diagrams in this image.
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