The pressure at equilibrium obtained upon $50\%$ dissociation of ${\mathrm{PCl}}_5$ at $250°\mathrm{C}$ is numerically ______ times of ${\mathrm{K}}_{\mathrm{P}.}$

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

The ratio of the partial pressure of ${\mathrm{O}}_2$ at equilibrium in the given reactions at same temperature is:

${\mathrm{Ag}}_2{\mathrm{O}}_{\left(\mathrm{s}\right)}\rightleftharpoons 2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}+{}_2{}^1\mathrm{O}_{2\left(\mathrm{g}\right)}$

$2{\mathrm{Ag}}_2{\mathrm{O}}_{\left(\mathrm{s}\right)}\rightleftharpoons 4{\mathrm{Ag}}_{\left(\mathrm{s}\right)}+{\mathrm{O}}_{2\left(\mathrm{g}\right)}$

At constant pressure, the addition of argon to, ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ will:

If the equilibrium constant for the reaction, ${\mathrm{P}}_{4\left(\mathrm{g}\right)}+6{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}\rightleftharpoons 4{\mathrm{PCl}}_{3\left(\mathrm{g}\right)}$ is $0.125$. The value of equilibrium for the reaction, $4{\mathrm{PCl}}_{3\left(\mathrm{g}\right)}\rightleftharpoons {\mathrm{P}}_{4\left(\mathrm{g}\right)}+6{\mathrm{Cl}}_{2\left(\mathrm{g}\right)}$ will be: