Solved: CHEMISTRY Question for NEET

NEET CHEMISTRYMedium

The following equilibrium constants are given: $N_2 + 3H_2 \rightleftharpoons 2NH_3$ ; $K_1$ $N_2 + O_2 \rightleftharpoons 2NO$ ; $K_2$ $H_2 + \frac{1}{2}O_2 \rightleftharpoons H_2O$ ; $K_3$ The equilibrium constant for the oxidation of $NH_3$ by oxygen to give NO is:

$\frac{K_2K_3^3}{K_1}$

$\frac{K_2K_3^2}{K_1}$

$\frac{K_2^2K_3}{K_1}$

$\frac{K_1K_2}{K_3}$

Step-by-Step Solution

The target reaction is the oxidation of $NH_3$ to NO: $2NH_3 + \frac{5}{2}O_2 \rightleftharpoons 2NO + 3H_2O$ This reaction can be obtained by adding the following reactions:

Reverse of reaction 1: $2NH_3 \rightleftharpoons N_2 + 3H_2$ ; $K'_1 = \frac{1}{K_1}$
Reaction 2: $N_2 + O_2 \rightleftharpoons 2NO$ ; $K_2$
Reaction 3 multiplied by 3: $3H_2 + \frac{3}{2}O_2 \rightleftharpoons 3H_2O$ ; $K'_3 = K_3^3$ Adding the three reactions, we get: $2NH_3 + \frac{5}{2}O_2 \rightleftharpoons 2NO + 3H_2O$ The equilibrium constant for this net reaction is the product of the individual equilibrium constants : $K = K'_1 \times K_2 \times K'_3 = \frac{1}{K_1} \times K_2 \times K_3^3 = \frac{K_2K_3^3}{K_1}$

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