Question

Given that the equilibrium constant for the reaction $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$
has a value of $278$ at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature?
$S{O}_{3\left(g\right)}\rightleftharpoons S{O}_{2\left(g\right)}+\frac{1}{2}{O}_{2\left(g\right)}$

• A. $6.0\times {10}^{-2}$
• B. $1.3\times {10}^{-5}$
• C. $1.8\times {10}^{-3}$
• D. $3.6\times {10}^{-5}$

Answer 1

The correct option is A $6.0\times {10}^{-2}$

${2SO}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2{SO}_3\left(g\right)K=278$ at $T$

Now for ${SO}_2+1/2O_2\rightleftharpoons {SO}_3\left(g\right)$ will have $\sqrt{K}$

$\Rightarrow {SO}_3\left(g\right)\rightleftharpoons {SO}_2\left(g\right)+1/2O_2\left(g\right)$ will have $1/\sqrt{K}$

$\frac{1}{\sqrt{278}}=6\times {10}^{-2}$