Question

Consider the following equilibrium in a closed container: $N_2{O}_4\left(g\right)\to 2N{O}_2\left(g\right)$ At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold true regarding the equilibrium constant $\left(K_p\right)$ and degree of dissociation $\alpha$?

• A. Neither Kp nor $K_p$ changes
  
• B. Both $K_p$ and $\alpha$ changes
• C. $K_p$ changes but $\alpha$ does not change
• D. $K_p$ does not change but $\alpha$ changes

Answer 1

The correct option is D $K_p$ does not change but $\alpha$ changes

$K_p$ does not change but $\alpha$ changes
$\to K_p$ of a reaction always remains fixed at a fixed temperature but extent of the reaction changes according to change in pressure conditions (if $\Delta n_g\ne 0$)