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Derivation of Kp and Kc

At 500K, th...

Question

At $500 K$ , the equilibrium constant for reaction ${c i s - C}_{2} H_{2} {C l}_{2} (g) ⇌ {t r a n s - C}_{2} H_{2} {C l}_{2} (g)$ is $0.6$ . At the same temperature, the equilibrium constant for the reaction ${t r a n s - C}_{2} H_{2} {C l}_{2} (g) ⇌ {c i s - C}_{2} H_{2} {C l}_{2} (g)$ , will be:

1.67

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0.6

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1.76

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1.64

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Solution

The correct option is A $1.67$
At $500 K$ , the equilibrium constant for reaction ${c i s - C}_{2} H_{2} {C l}_{2} (g) ⇌ {t r a n s - C}_{2} H_{2} {C l}_{2} (g)$ is $0.6$ . At the same temperature, the equilibrium constant for the reaction ${t r a n s - C}_{2} H_{2} {C l}_{2} (g) ⇌ {c i s - C}_{2} H_{2} {C l}_{2} (g)$ , will be
$\frac{1}{0.6} = 1.67$
$K = \frac{{t r a n s - C}_{2} H_{2} {C l}_{2} (g)}{{c i s - C}_{2} H_{2} {C l}_{2} (g)} = 0.6$
$K^{'} = \frac{{c i s - C}_{2} H_{2} {C l}_{2} (g)}{{t r a n s - C}_{2} H_{2} {C l}_{2} (g)} = \frac{1}{0.6} = 1.67$

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