The volume of the container containing a liquid and its vapours at a constant temperature is suddenly increased. What would be the effect of the change on vapour pressure?

For a reaction, 2NO _(g) + Br_{2 (g)}  $\leftrightharpoons$2NOBr _(g)

When 0.087 mol of NO and 0.0437 mol of Br₂ are mixed in a closed container at a constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The concentration of NO and Br₂ at equilibrium will be:

1. NO = 0.0352 mol; ${\mathrm{Br}}_2$= 0.0178 mol

2. NO = 0.352 mol; ${\mathrm{Br}}_2$= 0.178 mol

3. NO = 0.0634 mol; ${\mathrm{Br}}_2$= 0.0596 mol

4. NO = 0.634 mol; ${\mathrm{Br}}_2$= 0.596 mol

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

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

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