Question

At constant temperature, the equilibrium constant $\left(K_p\right)$ for the decomposition reaction
$N_2{O}_4\rightleftharpoons 2N{O}_2$ is expressed by $K_p=\left(4x^{2}P\right)/(1-x^2)$, where $P=$ pressure and $x=$ extent of decomposition. Which one of the following statements is false?

• A. $K_p$ increases with increase of $P$
• B. $K_p$ increases with increases of $T$
• C. $K_p$ increases with decrease of $x$
• D. $K_p$ remains constant with change in $P$ and $x$

Answer 1

Answer: (A), (C), (D)

$K_p$ increases with increase of $P$
$K_p$ increases with decrease of $x$
$K_p$ remains constant with change in $P$ and $x$

$K_P$ for a reaction at constant temperature remains constant. It depends only on temperature $T$. It is independent of $P$ & $x$. By Van't Hoff eqn :-

$\frac{dln{K}_P}{dT}=\frac{△H^0}{{RT}^2}$