Question

Consider the following system at equilibrium where AH = 18.8 kJ, and K-9.52x10-2, at 350 K CH_(g) + CCI(g) 2CH2Cl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of K. A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than K. B. is equal to Kc C. is less than K The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. A. increase. The number of moles of CCI, will: B. decrease. C. remain the same.

Answer 1

* untill and unless temperature is not changed then K_c does not change.

* value of Q_c is equal to K_c

* The reaction must remain the same it is already in equilbrium

* If reaction is neither going reverse nor forward no effect on concentration of CCl₄ it remains the same.
CHy (g) + Cely (g) 2 CH₂ C ₂ (g). Kc = [CH₂ C₂7² [CH] [Сcly) youme is reduced to Half then - cance of each species will be doubled.

Now Qc = [2 CH₂ CL] [2 CHA] [2ccly]. CH2Cl2) xxx [CMy] [ccly] (Qc - kc no effect on equilibrium. requcing youme Qc 7 Kc ? Reaction goes to deverge. Qc kc | Reaction goes to forward Qc - Kc ( no effect on equilbrium.