Question

$K_1$ and $K_2$ are equilibrium constant for reactions (1) and (2) $N_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO\left(g\right)......\left(1\right)$
$NO\left(g\right)\rightleftharpoons \frac{1}{2}{N}_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right).........\left(2\right)$
Then,

• A. $K_1=(\frac{1}{K_2}{)}^2$
• B. $K_1=L_2^2$
• C. $K_1=\frac{1}{K_2}$
• D. $K_1=(K_2{)}^0$

Answer 1

Answer: (A)

$K_1=(\frac{1}{K_2}{)}^2$

For reaction (1)
$K_1=\frac{[NO{]}^2}{\left[N_2\right]\left[O_2\right]}$
and for reaction (2)
$K_2=\frac{\left[N_2{]}^{\frac{1}{2}}\right[O_2{]}^{\frac{1}{2}}}{\left[NO\right]}$ therefore $K_1=\frac{1}{K_2^2}$