Consider the following system at equilibrium where Delta H degree - 111 kJ, and

Question

Consider the following system at equilibrium where Delta H degree - 111 kJ, and K_c = 6.30, at 723 K. 2NH_3 (g) N_2(g) + 3H_2 (g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of K_c increases. decreases. remains the same. The value of Q_c is greater than K_c. is equal to K_c. is less than K_c. 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. The number of moles of H_2 will: increase. decrease. remain the same.

Explanation / Answer

Kc remains the same, since it is a CONSTANT that depends only on T

Qc will change, since decrease of V will favour products, therefore Q increases (products increase)

the reaction must run forward to reestablish equilibrium

the number of H2 will increase, since it is favoured (products)

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