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Consider the following system at equilibrium where AH° = 111 kJ/mol, and Kc = 6.30, at 723 K. 2 NH3 (g) N₂ (g) + 3 H₂ (g) When 0.15 moles of NH3 (g) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc î The concentration of N₂ will ⒸK₁. The reaction must Orun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. C

Consider the following system at equilibrium where AH° = 111 kJ/mol, and Kc = 6.30, at 723 K. 2 NH3 (g) N₂ (g) + 3 H₂ (g) When 0.15 moles of NH3 (g) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc î The concentration of N₂ will ⒸK₁. The reaction must Orun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. C

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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 111 kJ/mol, and Kc = 6.30, at 723 K. 2 NH3 (g) N₂ (g) + 3 H₂ (g) When 0.15 moles of NH3 (g) are removed from the equilibrium system at constant temperature: The value of K The value of Qc ↑ The concentration of N₂ will Ⓒ KC. The reaction must Orun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium.
Transcribed Image Text:Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 111 kJ/mol, and Kc = 6.30, at 723 K. 2 NH3 (g) N₂ (g) + 3 H₂ (g) When 0.15 moles of NH3 (g) are removed from the equilibrium system at constant temperature: The value of K The value of Qc ↑ The concentration of N₂ will Ⓒ KC. The reaction must Orun in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium.
Expert Solution
Step 1: Relation between reaction quotient and equilibrium constant!

Answer:

  1. When QC=KC, system is at equilibrium.
  2. When QC<KC, system is not at equilibrium and in order to establish the equilibrium reaction has to move in forward direction, so that value of QC can increase and becomes equal to KC.
  3. When QC>KC, system is not at equilibrium and in order to establish the equilibrium reaction has to move in reverse direction, so that value of QC can decrease and becomes equal to KC.
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