The relation between equilibrium constant $K_p$ and $K_c$ is

For the reaction $PCl_5 \, (g) \rightleftharpoons PCl_3 \, (g) + Cl_2 \, (g)$,the two reaction constants $K_p$ and $K_c$ are related to each other by the expression

At a certain temperature in a $5\,L$ vessel,$2\,moles$ of carbon monoxide and $3\,moles$ of chlorine were allowed to reach equilibrium according to the reaction,$CO + Cl_2 \rightleftharpoons COCl_2$. At equilibrium,if $1\,mole$ of $CO$ is present,then the equilibrium constant $(K_c)$ for the reaction is:

Consider the reaction $N_{2}O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. The temperature at which $K_{C}=20.4$ and $K_{P}=600.1$ is ....... $K$. (Round off to the nearest integer).
[Assume all gases are ideal and $R=0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$]

For the reaction $C_{(s)} + CO_{2(g)} \rightleftharpoons 2CO_{(g)}$,at equilibrium,$P_{CO_2} = 2$ and $P_{CO} = 4$. The value of $K_p$ is:

For the reversible reaction in equilibrium
$N_{2(g)} + O_{2(g)} \underset{k_2}{\overset{k_1}{\longleftrightarrow}} 2NO_{(g)}$
If the rate constant for the forward reaction is $k_1 = 2.1 \times 10^{-3} \ s^{-1}$ and for the backward reaction is $k_2 = 4.2 \times 10^{-4} \ s^{-1}$,then the equilibrium constant $K_c$ for the above reaction is: