$SO_3(g) \rightleftharpoons SO_2(g)+ \frac{1}{2} O_2(g)$
is $K_c= 4.9 \times 10^{-2}.$ The value of $K_c$ for the reaction
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$
will be
$K_{c}=\frac{\left|S O_{2} \| O_{2}\right|^{1 / 2}}{\left|S O_{3}\right|}$
$=4.9 \times 10^{-2}$
On taking the square of the above reaction
$\frac{\left[S O_{2}\right]^{2}\left|O_{2}\right|}{\left[S O_{3}\right]^{2}}$
$=24.01 \times 10^{-4}$
now $K_{C}^{\prime}$
for $2 S O_{2}(g)+O_{2}(g) \rightleftharpoons 2 S O_{3}$
$=\frac{\left|S O_{3}\right|^{2}}{\left[S O_{2}\right]^{2}\left[O_{2}\right]}$
$=\frac{1}{24.01 \times 10^{-4}}$
$=416$
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$\mathrm{HF}, \mathrm{H}_2, \mathrm{H}_2 \mathrm{~S}, \mathrm{CO}_2, \mathrm{NH}_3, \mathrm{BF}_3, \mathrm{CH}_4, \mathrm{CHCl}_3, \mathrm{SiF}_4$, $\mathrm{H}_2 \mathrm{O}, \mathrm{BeF}_2$