If the equilibrium constant of the reaction $2 H I ⇌ H_{2} + I_{2}$ is $0.25$ , then the

equilibrium constant of the reaction $H_{2} + I_{2} ⇌ 2 H I$ would be

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Solution

The correct option is D
4.0

$K_{1}$ for reaction $2 H I ⇌ H_{2} + I_{2}$ is $0.25$ . $K_{2}$ for reaction $H_{2} + I_{2} ⇌ 2 H I$ will be
$K_{2} = \frac{1}{K_{1}} = \frac{1}{0.25}$ = $4$ . Because $2^{n d}$ reaction is reverse of $1^{s t}$ .

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Similar questions

If the equilibrium constant of the reaction $2 H I ⇌ H_{2} + I_{2}$ is $0.25$ , then the

equilibrium constant of the reaction $H_{2} + I_{2} ⇌ 2 H I$ would be

The equilibrium constant of the reaction 2HI ⇌ H₂ + I₂ is 0.25, the equilibrium constant of the reaction H₂ + I₂ ⇌ 2HI would be:

H_{2} + I_{2} ⇌ 2 H I

The equilibrium constant for the given reaction $H_{2} + I_{2} ⇌ 2 H I$ is correctly

given by expression

H_{2} + I_{2} ⇌ 2 H I

K

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