Consider the following gaseous equilibria with equilibrium constants $K_1$,and $K_2$ respectively.

$\begin{array}{l}{\mathrm{SO}}_2\left(\mathrm{g}\right)+1/2{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right)\\ 2{\mathrm{SO}}_3\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\end{array}$

The equilibrium constants are related as :

The first reaction is multiplied by 2 and reversed to obtain the second reaction. Hence, the value of the equilibrium constant is equal to the reciprocal of the square of the value of the equilibrium constant of the first reaction.

K₁​=[SO₂​][O₂​]/[SO₃​]​

K₂​=$\left[{\mathrm{so}}_3\right]/{\left[s{o}_2\right]}^2\left[o_2\right]$​=​$1/{\mathrm{K}}_1^2$

${\mathrm{k}}_1^2=1/{\mathrm{k}}_2$
correct answer is 1