${{\mathrm{I}}_2}_{\left(\mathrm{s}\right)}$ $+$ $5{{\mathrm{F}}_2}_{\left(\mathrm{g}\right)}$ $$ $\to 2{\mathrm{IF}}_{5\left(g\right)}$ $$

The equilibrium constant K_c expression for the above mentioned reaction is:

$1.$ ${\mathrm{K}}_{\mathrm{C}}=$ $\frac{{\left[{\mathrm{IF}}_5\right]}^2}{{\left[{\mathrm{F}}_2\right]}^5}$
$2.$ ${\mathrm{K}}_{\mathrm{C}}=$ $\frac{{\left[{\mathrm{IF}}_5\right]}^2}{{\left[{\mathrm{F}}_2\right]}^5\left[{\mathrm{I}}_2\right]}$
$3.$ ${\mathrm{K}}_{\mathrm{C}}$ $=\frac{{\left[{\mathrm{F}}_2\right]}^5\left[{\mathrm{I}}_2\right]}{{\left[{\mathrm{IF}}_2\right]}^2}$
$4.$ $$ ${\mathrm{K}}_{\mathrm{C}}$ $=\frac{{\left[{\mathrm{F}}_2\right]}^5}{{\left[{\mathrm{IF}}_5\right]}^2}$

${\mathrm{K}}_{{\mathrm{a}}_1},$ ${\mathrm{K}}_{{\mathrm{a}}_2}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_3}$ are the respective ionisation constants for the following reactions.
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HS}^{-}\)
\(\mathrm{HS}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{S}^{2-}\)
\(\mathrm{H}_2 \mathrm{~S} \rightleftharpoons 2 \mathrm{H}^{+}+\mathrm{S}^{2-}\)
The correct relationship between ${\mathrm{K}}_{{\mathrm{a}}_1},$ ${\mathrm{K}}_{{\mathrm{a}}_2}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_3}$ is:

Reaction quotient for the reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is given by , $\mathrm{Q}$ $=$ $\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$ .The reaction will proceed from right to left if K_c value is:

In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be: