Equilibrium constants $K_{1}$ and $K_{2}$ for the following equilibria are

$N O (g) + 0.5 O_{2} (g) \to K_{1} N O_{2} (g)$ and
$2 N O_{2} (g) \to K_{2} 2 N O (g) + O_{2} (g)$

$K_{2} = \frac{1}{K_{1}}$

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$K_{2} = K_{1}^{2}$

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$K_{2} = \frac{K_{1}}{2}$

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$K_{2} = \frac{1}{K_{1}^{2}}$

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Solution

The correct option is D
$K_{2} = \frac{1}{K_{1}^{2}}$

$K_{1} = \frac{[N O_{2}]}{[N O] [O_{2}]^{0.5}}$ and

$K_{2} = \frac{[N O]^{2} [O_{2}]}{[N O_{2}]^{2}}$

Or $K_{2} = \frac{1}{K_{1}^{2}}$

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Similar questions

Equilibrium constants $K_{1}$ and $K_{2}$ for the following equilibria are

$N O (g) + 0.5 O_{2} (g) \to K_{1} N O_{2} (g)$ and
$2 N O_{2} (g) \to K_{2} 2 N O (g) + O_{2} (g)$

Equilibrium constants $K_{1}$ and $K_{2}$ for the following equilibria are

$N O (g) + 0.5 O_{2} (g) \to K_{1} N O_{2} (g)$ and
$2 N O_{2} (g) \to K_{2} 2 N O (g) + O_{2} (g)$

K_{1}

K_{2}

N O (g) + \frac{1}{2} O_{2}_{1} {N O}_{2} (g)

2 {N O}_{2} (g)_{2} 2 N O (g) + O_{2} (g)

K_{1}

K_{2}

N O_{(g)} + \frac{1}{2} O_{2 (g)} ⇌ N O_{2 (g)}

2 N O_{2 (g)} ⇌ 2 N O_{(g)} + O_{2 (g)}

Two gaseous equilibria $S O_{2} (g) + 0.5 O_{2} (g) ⇌ S O_{3} (g)$ and

$2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)$ have equilibrium constants $K_{1}$ and $K_{2}$ respectively

at 298K. Which of the following relationships between $K_{1}$ and $K_{2}$ is correct

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