Question

The equilibrium constant ($K_c$) of the reaction $2S{O}_2+O_2\leftrightharpoons 2S{O}_3$, when the reaction is conducted in a one litre vessel was found to be $2.5\times {10}^{-3}$. If the reaction is conducted at the same temperature in a 2 litre vessel, then the value of $K_c$ is:

• A. $6.25\times {10}^{-3}$
• B. $1.25\times {10}^{-3}$
• C. $2.5\times {10}^{-3}$
• D. $5\times {10}^{-3}$

Answer 1

The correct option is C $2.5\times {10}^{-3}$

We are given that the equilibrium constant ($K_c$) of the reaction $2S{O}_2+O_2\leftrightharpoons 2S{O}_3$, when the reaction is conducted in a one litre vessel is $2.5\times {10}^{-3}$.

The magnitude of the equilibrium constant is not affected by the changes in concentrations of reactants and products, pressure and volume.

Hence, if the reaction is carried out in a $1$ litre vessel or in a $2$ litres vessel, the value of the equilibrium constant remains the same, i.e., $2.5\times {10}^{-3}$.