Question

Consider the two gaseous equilibrium involving $S{O}_2$ and the corresponding equilibrium constants at 299 K,

$S{O}_2\left(g\right)+1/2O_2\left(g\right)\rightleftharpoons S{O}_3\left(g\right);K_1$

$4S{O}_3\left(g\right)\rightleftharpoons 4S{O}_2\left(g\right)+2O_2\left(g\right);K_2$

The value of the equilibrium constant are related by :-

• A. $K_2=\frac{1}{{\left(K_1\right)}^4}$
• B. $K_2=K_1^4$
• C. $K_2={(\frac{1}{K_1})}^{1/4}$
• D. $K_2=\frac{1}{K_1}$

Answer 1

The correct option is A $K_2=\frac{1}{{\left(K_1\right)}^4}$

$S{O}_2\left(g\right)+1/2O_2\left(g\right)\rightleftharpoons S{O}_3\left(g\right);K_1$ ________(i)

$4S{O}_3\left(g\right)\rightleftharpoons 4S{O}_2\left(g\right)+2O_2\left(g\right);K_2$_______(ii)

2nd reaction can be obtained by reversing the first reaction and multiplying it by 4.

Hence, $K_1=(\frac{1}{K_2}{)}^4$

$\Rightarrow K_2=(\frac{1}{K_1}{)}^{1/4}$

Hence, option A is correct