For the reaction equilibrium, $2\mathrm{NOBr}\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)+{\mathrm{Br}}_2\left(\mathrm{g}\right),$ if ${\mathrm{P}}_{{\mathrm{Br}}_2}=\frac{\mathrm{P}}{9}$ at equilibrium and $\mathrm{P}$ is total pressure, then the ratio $\frac{{\mathrm{K}}_{\mathrm{P}}}{\mathrm{P}}$ is equal to: (assume that equilibrium was achieved starting with only $\mathrm{NOBr}$)

The value of ${\mathrm{K}}_{\mathrm{c}}$ for the reaction:

$\mathrm{A}+3\mathrm{B}\rightleftharpoons 2\mathrm{C} \mathrm{at} 400 °\mathrm{C}$ is $0.5 \mathrm{mol} {\mathrm{L}}^{-1}.$ Calculate the value of ${\mathrm{K}}_{\mathrm{P}}$ in $\mathrm{atm}$.

The volume of a closed reaction vessel in which the following equilibrium reaction occurs is halved.

$2{\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{O}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3 \left(\mathrm{g}\right)$

As a result,

Some reactions and their equilibrium constants given below :

${\mathrm{CuCl}}_4^{2-}+{\mathrm{Br}}^{-}\rightleftharpoons {\mathrm{CuCl}}_3{\mathrm{Br}}^{2-}+{\mathrm{Cl}}^{-} {\mathrm{K}}_1$

${\mathrm{CuCl}}_3{\mathrm{Br}}^{2-}+{\mathrm{Br}}^{-}\rightleftharpoons {\mathrm{CuCl}}_2{\mathrm{Br}}_2{}^{2-}+{\mathrm{Cl}}^{-} {\mathrm{K}}_2$

${\mathrm{CuCl}}_2{\mathrm{Br}}_2{}^{2-}+{\mathrm{Br}}^{-}\rightleftharpoons {\mathrm{CuClBr}}_3{}^{2-}+{\mathrm{Cl}}^{-} {\mathrm{K}}_3$

${\mathrm{CuClBr}}_3^{2-}+{\mathrm{Br}}^{-}\rightleftharpoons {\mathrm{CuBr}}_4^{2-}+{\mathrm{Cl}}^{-} {\mathrm{K}}_4$

The equilibrium constant, $\mathrm{K}$, for the reaction ${\mathrm{CuCl}}_4^{2-}+3{\mathrm{Br}}^{-}\rightleftharpoons {\mathrm{CuClBr}}_3^{2-}+3 {\mathrm{Cl}}^{-}$, is:

Consider the reactions:

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

(ii) ${\mathrm{N}}_2{\mathrm{O}}_4 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2 \left(\mathrm{g}\right)$

The addition of an inert gas at a constant volume: