Law of Chemical Equilibrium and Equilibrium Constants

At constant temperature, the equilibrium constant  $\left({\mathrm{K}}_{\mathrm{p}}\right)$ for the decomposition reaction  ${\mathrm{N}}_2{\mathrm{O}}_4\left(\text{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\text{g}\right)$  is expressed by ${\mathrm{K}}_{\mathrm{p}}=\frac{4{\mathrm{x}}^2}{1-{\mathrm{x}}^2}\mathrm{P}$ , where P = pressure, $\mathrm{x}$ = extent of decomposition. Which one of the following statements is true?

At constant temperature, the equilibrium constant  $\left(K_p\right)$ for the decomposition reaction  ${\mathrm{N}}_2{\mathrm{O}}_4\left(\text{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\text{g}\right)$  is expressed by ${\mathrm{k}}_{\mathrm{p}}=\frac{\left(4{\mathrm{x}}^2\mathrm{P}\right)}{(1-{\mathrm{x}}^2)}$ , where P = pressure, x = extent of decomposition. Which one of the following statements is true?

For the reversible reaction,  ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ at $500°\mathrm{C}$, the value of  ${\mathrm{K}}_{\text{p}}$ is  $1.44\times {10}^{-5}$ when partial pressure is measured in the atmosphere. The corresponding value of  ${\mathrm{K}}_{\text{c}}$, with concentration in $\mathrm{mol} {\mathrm{L}}^{-1}$, is: 

For the reversible reaction ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\text{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ at $\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}500°C$, the value of ${\mathrm{K}}_{\text{p}}$ is $1.44\times {10}^{-5}$ when partial pressure is measured in atmosphere. The corresponding value of ${\mathrm{K}}_{\text{c}}$, with concentration in $\mathrm{mol} {\mathrm{litre}}^{-1}$, is:

The Haber’s process for the formation of  ${\mathrm{NH}}_3$ at 298 K is

 ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3;\mathrm{\Delta H}=-46.0\mathrm{J}$.

Which of the following is the correct statement –

For the reversible reaction, ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\text{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ at $500°\mathrm{C}$ , the value of ${\mathrm{K}}_{\text{p}}$ is $1.44\times {10}^{-5}$, when partial pressure is measured in the atmosphere. The corresponding value of ${\mathrm{K}}_{\text{c}}$, with the concentration in $\mathrm{mole} {\mathrm{litre}}^{-1}$, is

For the chemical reaction  $\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}\mathrm{}3X\left(g\right)+\text{Y(g)}\rightleftharpoons X_{3}Y\left(g\right)$ , the amount of  $X_{3}Y$ at equilibrium is affected by –

For the reaction equilibrium,  ${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}\text{(g) }\underset{}{\rightleftharpoons }{\text{ 2NO}}_{\text{2}}\text{(g)}$ the concentrations of  ${\text{N}}_{\text{2}}{\text{O}}_{\text{4}}$ and  ${\text{NO}}_2$ at equilibrium are  $4.8\times 10^{-2}and1.2\times 10^{-2}mol{L}^{-1}$ respectively. The value of K_c for the reaction is –