Question

$K_1$ and $K_2$ are equilibrium constants for reaction (i) and (ii)

(i) $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)$

(ii)$NO\left(g\right)\rightleftharpoons N_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)$

• A. $K_1=(1/K_2{)}^2$
• B. $K_1=K_2^2$
• C. $K_1=1/K_2$
• D. $K_1=(K_2{)}^o$

Answer 1

Answer: (A)

$K_1=(1/K_2{)}^2$

$N_2+O_2\rightleftharpoons 2NO{K}_1$

$NO\rightleftharpoons \frac{1}{2}{N}_2+\frac{1}{2}{O}_2{K}_2$

The reaction is halved and reversed

$K_2=\sqrt{\frac{1}{K_1}}\Rightarrow K_1=\frac{1}{{K_2}^2}$