Question

For the reaction, $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$ at $300K$, the value of $\Delta G^o$ is $-690.9R.$

The equilibrium constant value for the reaction at that temperature is (R is gas constant)

• A. $10at{m}^{-1}$
• B. $10atm$
• C. $10$
• D. $1$

Answer 1

The correct option is A $10at{m}^{-1}$

For the reaction,
$2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right)$

Given that, $\Delta G^o=-690.9R,T=300K$

From the formula, $\Delta G^o=-RTlnK$

$-690.9R=-R\times 300\times InK$

or $lnk=\frac{690.9}{300}=2.303$

or $=2303logK=2303$

or $K={10}^1=10$

Unit of $K=(atm{)}^{\Delta n}=(atm{)}^{2-3}=(atm{)}^{-1}$

$\therefore K=10at{m}^{-1}$