AP Chemistry Question of the Day --14

Here comes the answer to question 13 I posted yesterday. The correct answer is C. 
The rates of the reaction, both forward and backward are affected by the concentration of the reactant (forward reaction) and product (backward reaction). Since initially, there was only PCl5 in the system, the forward reaction rate was at the maximum. The backward reaction rate was zero. As reaction goes, the concentration of PCl5 decreases and that of PCl3 and Cl2 increase, causing the forward reaction to slow down and the backward reaction to speed up. When the forward and backward reaction rate are the same, the equilibrium is achieved. The chemical equilibrium is a dynamic equilibrium and the rate will never be 0. 

Following is Question 14 of the series. It is in continuation with question 12 and 13. 

13. PCl5(g) decomposes into PCl3(g) and Cl2(g) according to the equation above. A pure sample of PCl5(g) is placed in a rigid, evacuated 1.00 L container. The initial pressure of the PCl5(g) is 1.00 atm. The temperature is held constant until the PCl5(g) reaches equilibrium with its decomposition products. The figures below show the initial and equilibrium conditions of the system. Which of the following statements about Kp, the equilibrium constant for the reaction, is correct?

(A) Kp > 1
(B) Kp < 1
(C) Kp = 1
(D) It cannot be determined whether Kp > 1, Kp < 1, or Kp = 1 without additional information

I will post the answer and explanation tomorrow.

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