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Q.

For the reaction, $2 {NO}_{2} (g) ⇌ 2 NO (g) + O_{2} (g)$ , $K_{c} = 1 .8 \times 10^{- 6}$ at 185°C. At 185°C, the K_c for $NO (g) + \frac{1}{2} O_{2} (g) ⇌ {NO}_{2} (g)$ is :

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a

1.95 x 10^-3

b

1.95 x 10³

c

0.9 x 10⁶

d

7.5 x 10²

answer is B.

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Detailed Solution

$\begin{array}{l} K_{c_{1}} = \frac{[NO]^{2} [O_{2}]}{{[{NO}_{2}]}^{2}} = 1 .8 \times 10^{- 6} \\ Also, K_{c_{2}} = \frac{[{NO}_{2}]}{[NO] {[O_{2}]}^{1 / 2}} \\ K_{c_{1}} = \frac{1}{K_{c_{2}}^{2}} \\ or 1 .8 \times 10^{- 6} = \frac{1}{K_{c_{2}}^{2}} \\ ∴ K_{c_{2}} = 7 .5 \times 10^{2} \end{array}$

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For the reaction, 2NO2(g)⇌2NO(g)+O2(g), Kc=1.8×10−6 at 185°C. At 185°C, the Kc for NO(g)+12O2(g)⇌NO2(g) is :