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Consider the following system at equilibrium where AH = 108 kJ, and K = 0.0129, at 600 K: COC12 (9) CO(g) + Cl₂ (g) If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke Oincreases Odecreases Oremains the same Visited 9 The value of Qc Ois greater than Ke Ois equal to Ke Ois less than Ke The reaction must Orun in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. Oremain the same. It is already at equilibrium. The number of moles of Cl₂ will Oincrease decrease Oremain the same

Consider the following system at equilibrium where AH = 108 kJ, and K = 0.0129, at 600 K: COC12 (9) CO(g) + Cl₂ (g) If the VOLUME on the equilibrium system is suddenly increased at constant temperature: The value of Ke Oincreases Odecreases Oremains the same Visited 9 The value of Qc Ois greater than Ke Ois equal to Ke Ois less than Ke The reaction must Orun in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. Oremain the same. It is already at equilibrium. The number of moles of Cl₂ will Oincrease decrease Oremain the same

Chemistry
Chemistry
10th Edition
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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**Educational Website Transcription** --- **Equilibrium System Analysis** Consider the following system at equilibrium where ΔH° = 108 kJ and Kc = 0.0129, at 600 K: \[ \text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g) \] **Scenario: Sudden Increase in Volume at Constant Temperature** 1. **Effect on the Equilibrium Constant (Kc)**: - The value of Kc: - ☐ Increases - ☐ Decreases - ☑ Remains the same 2. **Effect on the Reaction Quotient (Qc)**: - The value of Qc: - ☐ Is greater than Kc - ☑ Is equal to Kc - ☐ Is less than Kc 3. **Reaction Direction**: - The reaction must: - ☐ Run in the forward direction to reestablish equilibrium. - ☑ Run in the reverse direction to reestablish equilibrium. - ☐ Remain the same. It is already at equilibrium. 4. **Change in Moles of Cl2**: - The number of moles of Cl2 will: - ☐ Increase - ☑ Decrease - ☐ Remain the same **Note**: Graphs or diagrams are not present in the context of this text. --- **Resources**: Cengage Learning | Cengage Technical Support
Transcribed Image Text:**Educational Website Transcription** --- **Equilibrium System Analysis** Consider the following system at equilibrium where ΔH° = 108 kJ and Kc = 0.0129, at 600 K: \[ \text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g) \] **Scenario: Sudden Increase in Volume at Constant Temperature** 1. **Effect on the Equilibrium Constant (Kc)**: - The value of Kc: - ☐ Increases - ☐ Decreases - ☑ Remains the same 2. **Effect on the Reaction Quotient (Qc)**: - The value of Qc: - ☐ Is greater than Kc - ☑ Is equal to Kc - ☐ Is less than Kc 3. **Reaction Direction**: - The reaction must: - ☐ Run in the forward direction to reestablish equilibrium. - ☑ Run in the reverse direction to reestablish equilibrium. - ☐ Remain the same. It is already at equilibrium. 4. **Change in Moles of Cl2**: - The number of moles of Cl2 will: - ☐ Increase - ☑ Decrease - ☐ Remain the same **Note**: Graphs or diagrams are not present in the context of this text. --- **Resources**: Cengage Learning | Cengage Technical Support
**Chemical Equilibrium Analysis** Consider the following system at equilibrium where \( \Delta H^\circ = 10.4 \, \text{kJ} \), and \( K_c = 0.0180 \), at 698 K: \[ 2HI(g) \rightleftharpoons H_2(g) + I_2(g) \] ### Problem Statement If the **volume** of the equilibrium system is suddenly increased at constant temperature: 1. **The value of \( K_c \):** - Increases - Decreases - Remains the same 2. **The value of \( Q_c \):** - Is greater than \( K_c \) - Is equal to \( K_c \) - Is less than \( K_c \) 3. **The reaction must:** - Run in the forward direction to reestablish equilibrium. - Run in the reverse direction to reestablish equilibrium. - Remain the same. It is already at equilibrium. 4. **The number of moles of \( I_2 \) will:** - Increase - Decrease - Remain the same ### Explanation When the volume of a gaseous equilibrium system is increased at constant temperature, the equilibrium will shift in the direction that produces more moles of gas. This change affects the reaction quotient \( Q_c \) in comparison to the equilibrium constant \( K_c \). Understanding these impacts helps in predicting the shift in equilibrium and the changes in concentrations or pressures of the involved gases. For further learning, explore the principles of Le Chatelier's Principle and its application to changes in pressure and volume.
Transcribed Image Text:**Chemical Equilibrium Analysis** Consider the following system at equilibrium where \( \Delta H^\circ = 10.4 \, \text{kJ} \), and \( K_c = 0.0180 \), at 698 K: \[ 2HI(g) \rightleftharpoons H_2(g) + I_2(g) \] ### Problem Statement If the **volume** of the equilibrium system is suddenly increased at constant temperature: 1. **The value of \( K_c \):** - Increases - Decreases - Remains the same 2. **The value of \( Q_c \):** - Is greater than \( K_c \) - Is equal to \( K_c \) - Is less than \( K_c \) 3. **The reaction must:** - Run in the forward direction to reestablish equilibrium. - Run in the reverse direction to reestablish equilibrium. - Remain the same. It is already at equilibrium. 4. **The number of moles of \( I_2 \) will:** - Increase - Decrease - Remain the same ### Explanation When the volume of a gaseous equilibrium system is increased at constant temperature, the equilibrium will shift in the direction that produces more moles of gas. This change affects the reaction quotient \( Q_c \) in comparison to the equilibrium constant \( K_c \). Understanding these impacts helps in predicting the shift in equilibrium and the changes in concentrations or pressures of the involved gases. For further learning, explore the principles of Le Chatelier's Principle and its application to changes in pressure and volume.
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