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Stability of Carbocation

At 500 K, the...

Question

At $500 K$ , the equilibrium constant for $cis - C_{2} H_{2} C l_{2} (g) ⇋ trans - C_{2} H_{2} C l_{2} (g)$ is $0.6$ . At the same temperature, the equilibrium constant for the reaction, $trans - C_{2} H_{2} C l_{2} (g) ⇋ cis - C_{2} H_{2} C l_{2} (g)$ will be:

0.66

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1.67

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0.76

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2.6

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Solution

The correct option is B $1.67$
Given, the equlibrium constant for the reaction
$cis - C_{2} H_{2} C l_{2} (g) ⇋ trans - C_{2} H_{2} C l_{2} (g)$ is $K_{C} = 0.6$
So, the equlibrium constant for the reaction
$trans - C_{2} H_{2} C l_{2} (g) ⇋ cis - C_{2} H_{2} C l_{2} (g)$
$K_{C}^{'} = \frac{1}{K_{e}} = \frac{1}{0.6} = 1.67$

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