Consider the following system at equilibrium where Delta H degree = 182 kJ, and
ID: 498135 • Letter: C
Question
Consider the following system at equilibrium where Delta H degree = 182 kJ, and K_c = 7.00 times 10^-5, at 673 K. NH_4 I(s) NH_3 (g) + HI(g) When some moles of NH_4 I(s) are removed from the equilibrium system at constant temperature: the value of K_c __ A. increases. B. decreases. C. remains the same. the value of Q_c __ A. is greater than K_c. B. is equal to K_c. C. is less than K_c. the reaction must: ___ A. run in the forward direction to restablish equilibrium. B. run in the reverse direction to restablish equilibrium. C. remain the same. It is already at equilibrium. the concentration of NH_3 will: __ A. increase. B. decrease. C. remain the same.Explanation / Answer
The equilibrium constant remains unchanged
The vlue of Qc increases because we are removing the reactant i.e., the denominator term is less so Qc value increases.
By removing of NH4I, the equilibrium run in the reverse direction to reestablish equilibrium
[NH3] decreases by removing of NH4I because to reestablish the equilibrium the reaction has to move to backward ie., [NH3] decreases