For which of the following reactions, the degree of dissociation cannot be calculated from the vapour density data.

$\mathrm{I}. 2\mathrm{HI} \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2 \left(\mathrm{g}\right)+{\mathrm{I}}_2 \left(\mathrm{g}\right)$

$\mathrm{II}. 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2 \left(\mathrm{g}\right)+3{\mathrm{H}}_2 \left(\mathrm{g}\right)$

$\mathrm{III}. 2\mathrm{NO} \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{N}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)$

$\mathrm{IV}. {\mathrm{PCl}}_5 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3 \left(\mathrm{g}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)$

For ${\mathrm{NH}}_4\mathrm{HS}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)$, if${\mathrm{K}}_{\mathrm{P}}=64 {\mathrm{atm}}^2$, the equilibrium pressure of the mixture is

Given equilibrium constants for the following reactions at $1200°\mathrm{C}$.

$$\begin{gathered} \mathrm{C}\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{CO}\left(\mathrm{g}\right), {\mathrm{K}}_{{\mathrm{P}}_1}=1.47\times {10}^3 \\ \mathrm{CO}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right), {\mathrm{K}}_{{\mathrm{P}}_2}=2\times {10}^6 \end{gathered}$$

Calculate ${\mathrm{K}}_{\mathrm{P}}$ for the reaction$\mathrm{C} \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2 \left(\mathrm{g}\right)$.

High pressure and low temperature are the favourable conditions for the formation of product for the gaseous phase reaction, 

$\mathrm{xA}\rightleftharpoons \mathrm{yB}+\mathrm{zC}, ∆\mathrm{H}=-\mathrm{x} \text{kcal}$. Hence,

The exothermic formation of ${\mathrm{ClF}}_3$ is represented by the equation,

${\mathrm{Cl}}_2 \left(\mathrm{g}\right)+3{\mathrm{F}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{ClF}}_3 \left(\mathrm{g}\right); ∆\mathrm{H}=-329\mathrm{kJ}$.

Which of the following will increase the quantity of ${\mathrm{ClF}}_3$ in an equilibrium mixture of ${\mathrm{Cl}}_2$, ${\mathrm{F}}_2$ and ${\mathrm{ClF}}_3$?

In the system $\mathrm{AB}\left(\mathrm{s}\right)\rightleftharpoons \mathrm{A}\left(\mathrm{g}\right)+\mathrm{B}\left(\mathrm{g}\right)$, doubling the quantity of $\mathrm{AB}\left(\mathrm{s}\right)$ would