Vapour density of ${\mathrm{N}}_2{\mathrm{O}}_4$, which dissociated according to the equation ${\mathrm{N}}_2{\mathrm{O}}_4 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2 \left(\mathrm{g}\right)$, is $25.67$ at $100°\mathrm{C}$ and pressure of $1 \mathrm{atm}$. Calculate the degree of dissociation and ${\mathrm{K}}_{\mathrm{p}}$ for the reaction.

Equilibrium constant $\left({\mathrm{K}}_{\mathrm{p}}\right)$ for the reaction, $2{\mathrm{H}}_2\mathrm{S} \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{H}}_2 \left(\mathrm{g}\right)+{\mathrm{S}}_{ 2} \left(\mathrm{g}\right)$ is $0.0118$ at $1065°\mathrm{C}$ and the heat of dissociation is $42.4 \mathrm{kcal}$. Find equilibrium constant $\text{ at }1132°\mathrm{C}$.

In the gaseous reaction $2\mathrm{A}+\mathrm{B}\rightleftharpoons {\mathrm{A}}_2\mathrm{B}, \mathrm{\Delta G}°=1200$ $\mathrm{cal}$ at $227°\mathrm{C}.$ What total pressure would be necessary to produce $60\%$ conversion of $\mathrm{B}$ into ${\mathrm{A}}_2\mathrm{B}$ when $2: 1$ mixture is used?

Equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the equilibrium,

$\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right)\text{ is }0·45\text{ at }200°\mathrm{C}$

One litre of a container contains $0·2$ $\mathrm{mole}$ of $\mathrm{A}, 0·3$ $\mathrm{mole}$ of $\mathrm{B}$ and $0·3$ $\mathrm{mole}$ of $\mathrm{C}$ at the equilibrium. Calculate the new equilibrium concentrations of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ if the volume of the container is doubled.

Equilibrium constant ${\mathrm{K}}_{\mathrm{c}}$ for the equilibrium,

$\mathrm{A} \left(\mathrm{g}\right)\rightleftharpoons \mathrm{B} \left(\mathrm{g}\right)+\mathrm{C} \left(\mathrm{g}\right)$ is $0.45$at $200°\mathrm{C}$

One litre of a container contains $0.2$ $\mathrm{mole}$ of $\mathrm{A}, 0.3$ $\mathrm{mole}$ of $\mathrm{B}$ and $0.3$ $\mathrm{mole}$ of $\mathrm{C}$ at the equilibrium. Calculate the new equilibrium concentrations of $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ if the volume of the container is halved at $200°\mathrm{C}$.

A $2 \mathrm{litre}$ vessel contains $0.48 \mathrm{mole}$ of ${\mathrm{CO}}_2, 0.48$ $\mathrm{mole}$ of ${\mathrm{H}}_2, 0.96$ $\mathrm{mole}$ of ${\mathrm{H}}_2\mathrm{O}$ and $0.96 \mathrm{mole}$ of $\mathrm{CO}$ at equilibrium.

$\left\{{\mathrm{CO}}_2 \left(\mathrm{g}\right)+{\mathrm{H}}_2 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)+\mathrm{CO} \left(\mathrm{g}\right)\right\}$

A $2 \mathrm{litre}$ vessel contains $0.48 \mathrm{mole}$ of ${\mathrm{CO}}_2, 0.48$ $\mathrm{mole}$ of ${\mathrm{H}}_2, 0.96$ $\mathrm{mole}$ of ${\mathrm{H}}_2\mathrm{O}$ and $0.96 \mathrm{mole}$ of $\mathrm{CO}$ at equilibrium. $\left\{{\mathrm{CO}}_2 \left(\mathrm{g}\right)+{\mathrm{H}}_2 \left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)+\mathrm{CO} \left(\mathrm{g}\right)\right\}$

A $2-\mathrm{litre}$ vessel contains$0.48 \mathrm{mole}$ ${\mathrm{CO}}_2, 0.48$ $\mathrm{mole}$ of ${\mathrm{H}}_2, 0.96$ $\mathrm{mole}$ of ${\mathrm{H}}_2\mathrm{O}$ and $0.96 \mathrm{mole}$ of equilibrium.

$\left\{{\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)\right\}$

How many $\mathrm{moles}$ of ${\mathrm{H}}_2\mathrm{O}$ must be removed to bring the $\mathrm{CO}$ concentration to $0.60 \mathrm{M}?$