SbCl5 (g) ⇔ SbCl3 (g) + Cl2 (g) An 89.7 gram sample of liquid SbCL5 is placed in an evacuated 15.0 liter rigid container. As the container is heated to 500 K, the sample vaporizes completely and starts to decompose according to the equation above. The decomposition is endothermic.

a. Write the equilibrium constant expression, Kc, for the reaction above.

b. When the SbCl5 vapor completely vaporizes at 500 K, what is the molarity before it decomposes?

c. When the system has reached equilibrium at 500 K, the total number of moles of gas in the container is 0.387. Calculate the number of moles of each gas at equilibrium in the container at 500 K.

d. Calculate the equilibrium constant, Kc.