The vapour density of equilibrium mixture for $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$ is 28.75 at 1 atm. This mixture is allowed to diffuse out for 10 seconds. Calculate the $K_p$ of the reaction after 10 seconds.

Q. For the reaction, $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right),△H=57.49{\text{kJ mol}}^{-1}$.
With the increase in temperature, the vapour density of the equilibrium mixture:

Q. Vapour density of $N_2{O}_4$ which dissciates according to teh equilibrium $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$ is $25.67$ at ${100}^{o}C$ and a pressure of $1atm$. Calculate the degree dissociatrion for the reaction.

Q. The density of an equilibrium mixture of $N_2{O}_4$ and $N{O}_2$ at 1 atm and 346 K is 1.8 g/L. Calculate $K_C$ for the reaction:

Q. For the equilibrium $N_2{O}_4\left(g\right)\rightleftharpoons 2N{O}_2\left(g\right)$, mark the correct option that shows the correct relationship of the degree of dissociation - ${}^{\prime }{\alpha }^{\prime }$ with $D/d$; where $D$ is vapour density of $N_2{O}_4$ and $d$ is vapour density of equilibrium mixture.