Consider the following reaction: Ni(CO)4 (g) <---> Ni (s) + 4CO (g) Kc= 0.0309.

Question

Consider the following reaction:

Ni(CO)4 (g) <---> Ni (s) + 4CO (g)

Kc= 0.0309. A mixture of Ni(CO)4 (g) and CO (g), each with a concentration of 0.800 M, and an excess of Ni (s) were confined in a 1.0 L container at 300 K. Which of the following is true?

(a) Ni (s) is formed

(b) Ni(CO)4 (g) forms until equilibrium is reached

(c) some Ni(CO)4 (g) decomposes to CO (g) and Ni (s)

(d) no change occurs since we are at equilibrium

(e) Kc changes to 0.51

I know that the correct answer is (b), but I want to know why the correct answer is (b)

Explanation / Answer

Kc = 0.0309 < 1

So the equilibrium will shift to left...

Also, Ni is in excess...which will drive the reaction towards left...So NiCO4 will be formed until new equilibrium is reached...

Answer : B

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