$6$ moles of ${\mathrm{PCl}}_5$ were heated in a closed vessel of $2$ liter capacity. At equilibrium, $20\%$ of ${\mathrm{PCl}}_5$ is dissociated into ${\mathrm{PCl}}_3$ and ${\mathrm{Cl}}_2$. What is the value of the equilibrium constant?

${\mathrm{N}}_2{\mathrm{O}}_4\rightleftharpoons 2{\mathrm{NO}}_2$

Decomposition of ${\mathrm{N}}_2{\mathrm{O}}_4$ to ${\mathrm{NO}}_2$ is carried out at $280 \mathrm{K}$ and at equilibrium, $0.4 \mathrm{mole}$ of ${\mathrm{N}}_2{\mathrm{O}}_4$ and $4\times {10}^{-3} \mathrm{mole}$ of ${\mathrm{NO}}_2$ are present in $2 \text{litre}$ solution. What is the equilibrium constant for the reaction?

A gaseous phase reaction is allowed to attain equilibrium as:

$\mathrm{A}\left(\mathrm{g}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{g}\right)+\mathrm{C}\left(\mathrm{g}\right)$

At constant pressure $\mathrm{P}$, the partial pressure of $\mathrm{A}$ at equilibrium is $0.5 \mathrm{P}$. Then what will be the value of ${\mathrm{K}}_{\mathrm{p}}$?

$0.6$mole each of ${\mathrm{H}}_2$ and ${\mathrm{I}}_2$ react in a $10$ liter flask at ${500}^{°}\mathrm{C}$. What is the amount of unreacted ${\mathrm{I}}_2$ at equilibrium for the reaction?

${\mathrm{H}}_2 +{\mathrm{I}}_2 \rightleftharpoons 2\mathrm{HI}$ $({\mathrm{K}}_{\mathrm{c}}=64)$

$2{\mathrm{CO}}_2 \rightleftharpoons 2\mathrm{CO} +{\mathrm{O}}_2$

At $3000 \mathrm{K}$, the equilibrium pressures of ${\mathrm{CO}}_2$, $\mathrm{CO}$ and ${\mathrm{O}}_2$ are $6 \mathrm{atm}, 4 \mathrm{atm}$ and $2 \mathrm{atm}$ respectively. Find out ${\mathrm{K}}_{\mathrm{p}}$ for the above reaction.