Consider the following system at equilibrium where del H degree = -16.1 kJ, and

Question

Consider the following system at equilibrium where del H degree = -16.1 kJ, and K_c = 154, at 298 K. 2NO(g) + Br_2(g) implies 2NOBr(g) When 0.22 moles of Br2(g) are removed from the equilibrium system at constant temperature: the value of K_c A. increases. decreases. remains the same. the value of Q_c is greater than 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 concentration of NO will: increase. decrease. remain the same.

Explanation / Answer

1)Kc remains cnstant

2)Qc is greater than Kc

3)B

4)A

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