# At 500 K, the equilibrium constant, Kc, for the following reaction is 5.$\frac{1}{2} H_{2} (g) + \frac{1}{2} I_{2} (g) \rightleftharpoons HI (g)$ What would be the equilibrium constant  for the reaction $2HI (g)\rightleftharpoons H_{2} (g) + I_{2} (g)$(i) 0.04(ii) 0.4(iii) 25(iv) 2.5

The answer is the option (i) 0.04

Explanation: If the given equation is multiplied by 2, the equilibrium constant for the new equation will be squared, and on reversing the reaction the value of the equilibrium constant is reciprocated. Thus

For the required reaction equation

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