The equilibrium constant (KC) for the reaction N2(g) + O2(g) → 2NO(g) at temperature T is 4 × 10–4. The value of KC for the reaction, NO(g) → 1/2N2(g) + 1/2O2(g) at the same temperature is :

Engineering

Chemistry

Equilibrium Constant and Mass Action Law

Question

The equilibrium constant (K_C) for the reaction

N₂(g) + O₂(g) → 2NO(g)

at temperature T is 4 × 10^–4. The value of K_C for the reaction,

NO(g) → 1/2N₂(g) + 1/2O₂(g)

at the same temperature is :

2.5 × 10²

0.02

4 × 10^–4

50.0

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N₂(g) + O₂(g) $\overset{}{\to}$ 2NO(g) ; k₁ = 4 × 10^–4

NO(g) $\overset{}{\to}$ 1/2N₂(g) + 1/2 O₂(g); k₂ =?

$k_{2} = \frac{1}{\sqrt{k_{1}}} = 50$

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