$40\%$ of a mixture of $2$ moles of ${\mathrm{N}}_2$ and $6$ moles of ${\mathrm{H}}_2$ react to give ${\mathrm{NH}}_3$ according to the equation ${\mathrm{N}}_2 \left(\mathrm{g}\right)+3{\mathrm{H}}_2 \left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3 \left(\mathrm{g}\right)$ at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases are

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

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 $\left[\mathrm{A}\right]=\left[\mathrm{B}\right]=\left[\mathrm{C}\right]=3\times {10}^{-4} \mathrm{M}$

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].