Consider the following gaseous equilibria with equilibrium constants K 1 and K 2 respectively- SO - 2 g -1-2 O - 2 g - rightleftharpoons SO - 3 g SO - 3 g -2 SO - 2 g - O - 2 g The equilibrium constants are related as-A- K1-K2B- K2-K12C- K2-1-K12D- K2-1-K1

The correct option is C K_1=[SO_3]/[SO_2][O_2]^1/2 K_2=[SO_2]^2[O_2]/[SO_3]^2 K_1^2=[SO_3]^2/[SO_2]^2[O_2] hence K_2=1/K_1^2 ...

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Effective Equilibrium Constant

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Consider the following gaseous equilibria with equilibrium constants $K_{1}$ and $K_{2}$ respectively.
$S O_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ S O_{3} (g) 2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)$
The equilibrium constants are related as :

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S O_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ S O_{3} (g)

2 S O_{3} (g) ⇌ 2 S O_{2} (g) + O_{2} (g)

K_{1}

K_{2}

298 K

K_{1}

K_{2}

For the two gaseous reactions (i) and (ii), at $25^{\circ} C$

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

(ii) $2 N O_{2} (g) ⇌ 2 N O (g) + O_{2} (g)$ ,

The equilibrium constants are $K_{1}$ and $K_{2}$ respectively are related as:

For the two gaseous reactions (i) and (ii), at $25^{0} C$

$(i) N O (g) + \frac{1}{2} O_{2} (g) ⟵ N O_{2} (g)$

$(i i) 2 N O_{2} (g) ⟵ 2 N O (g) + O_{2} (g)$ ,

The equilibrium constants are $K_{1}$ and $K_{2}$ respectively. these two constants are related as:

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

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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