The vapour density of a sample ${\mathrm{N}}_2{{\mathrm{O}}_4}_{\left(\mathrm{g}\right)}$ is $40$ at $10 \mathrm{atm}$. Calculate the ${\mathrm{K}}_{\mathrm{P}}$ for the reaction.

For the following reaction, ${\mathrm{K}}_{\mathrm{c}}=2\times {10}^{-3}$

$2 \mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C}$

Identify the correct statement for the reaction when $\left[\mathrm{A}\right]=\left[\mathrm{B}\right]=\left[\mathrm{C}\right]=3\times {10}^{-4} \mathrm{M}$

At $\mathrm{T}\left(\mathrm{K}\right)$, for the gaseous reaction
$2 \mathrm{A}\rightleftharpoons \mathrm{B}+\mathrm{C},{\mathrm{K}}_{\mathrm{C}}$ is $2\times {10}^{-3}$

at a given time the composition of reaction mixture is $\left[\mathrm{A}\right]=\left[\mathrm{B}\right]=\left[\mathrm{C}\right]=3.0\times {10}^{-4}\mathrm{M},$the state of the reaction is

The reaction quotient $\left(\mathrm{Q}\right)$ for the reduction of ${\mathrm{O}}_2$ to ${\mathrm{H}}_2\mathrm{O}$ in acid solution,
${\mathrm{O}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+4{\mathrm{e}}^{-}⟶2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ is,
[where, ${\mathrm{\alpha }}_{{\mathrm{H}}^{+}}=$ activity of ${\mathrm{H}}^{+},{\mathrm{p}}_{{\mathrm{O}}_2}=$ pressure of ${\mathrm{O}}_2$ when it is present in the reaction, $\mathrm{p}°=$ pressure of ${\mathrm{O}}_2$ at standard state].

Vapour density of the equilibrium mixture of ${\mathrm{NO}}_2$ and ${\mathrm{N}}_2{\mathrm{O}}_4$ is found to be $38.33$: for the equilibrium ${\mathrm{N}}_2{\mathrm{O}}_4 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2 \left(\mathrm{g}\right)$.

Calculate: degree of dissociation.