For the reaction, ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$, the value of $\mathrm{K}$ is$50$ at$400 \mathrm{K}$ and$1700$ at$500 \mathrm{K}$. Which of the following option(s) is/are correct?

(a) ${{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons 2{\mathrm{NO}}_{\left(\mathrm{g}\right)}; {\mathrm{K}}_1$
(b) $\left(\frac{1}{2}\right){{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+\left(\frac{1}{2}\right){{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons \mathrm{NO}\left(\mathrm{g}\right); {\mathrm{K}}_2$
(c) $2{{\mathrm{NO}}_2}_{\left(\mathrm{g}\right)}\rightleftharpoons {{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+{{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}; {\mathrm{K}}_3$
(d) ${\mathrm{NO}}_{\left(\mathrm{g}\right)}\rightleftharpoons \left(\frac{1}{2}\right){{\mathrm{N}}_2}_{\left(\mathrm{g}\right)}+\left(\frac{1}{2}\right){{\mathrm{O}}_2}_{\left(\mathrm{g}\right)}; {\mathrm{K}}_4$

The correct relation between ${\mathrm{K}}_1, {\mathrm{K}}_2, {\mathrm{K}}_3$ and ${\mathrm{K}}_4$ is/are

For the reaction involving the oxidation of ammonia by oxygen to form nitric oxide and water vapour, the equilibrium constant has the units $(\mathrm{bar}{)}^{\mathrm{n}}$. Then, $\mathrm{n}$ is:

Consider the reaction: $2{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}+2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\rightleftharpoons 4{\mathrm{HCl}}_{\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}, \mathrm{\Delta H}°=+133 \mathrm{kJ}$.    $$
The four gases, ${\mathrm{Cl}}_2, {\mathrm{H}}_2\mathrm{O}, \mathrm{HCl}$ and ${\mathrm{O}}_2,$ are mixed and the reaction is allowed to come to equilibrium. State and explain the effect (increase, decrease, no change) of the operation in the left column (below) and the equilibrium value of the quantity in the right column. Each operation is to be considered separately. The temperature and volume are constant unless stated otherwise.

Increasing the volume of the container _________ number of moles of ${\mathrm{H}}_2\mathrm{O}$.

Consider the reaction:
$2{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}+2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\rightleftharpoons 4{\mathrm{HCl}}_{\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}, \mathrm{\Delta H}°=+133 \mathrm{kJ}$    $$
The four gases, ${\mathrm{Cl}}_2, {\mathrm{H}}_2\mathrm{O}, \mathrm{HCl}$ and ${\mathrm{O}}_2,$ are mixed and the reaction is allowed to come to equilibrium. State and explain the effect (increase, decrease, no change) of the operation in the left column (below) and the equilibrium value of the quantity in the right column. Each operation is to be considered separately. The temperature and volume are constant unless stated otherwise.

Adding ${\mathrm{O}}_2$ __________ number of moles of ${\mathrm{H}}_2\mathrm{O}$

Consider the reaction:
$2{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}+2{\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}\rightleftharpoons 4{\mathrm{HCl}}_{\left(\mathrm{g}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}, \mathrm{\Delta H}°=+133 \mathrm{kJ}$    $$
The four gases, ${\mathrm{Cl}}_2, {\mathrm{H}}_2\mathrm{O}, \mathrm{HCl}$ and ${\mathrm{O}}_2,$ are mixed and the reaction is allowed to come to equilibrium. State and explain the effect (increase, decrease, no change) of the operation in the left column (below) on the equilibrium value of the quantity in the right column. Each operation is to be considered separately. The temperature and volume are constant unless stated otherwise.

Adding ${\mathrm{O}}_2$ ___________ number of moles of $\mathrm{HCl}$.