For the following reaction in gaseous phase $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,$K_p/K_c$ is

The value of $K_{C}$ for the equilibrium reaction: $CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ at $T \ K$ is $0.036$. If the equilibrium concentration of $CO_{2(g)}$ is $0.004 \ M$,the concentration of $CO_{(g)}$ in $mol \ L^{-1}$ is:

For the reaction $MgCO_{3(s)} \rightleftharpoons MgO_{(s)} + CO_{2(g)}$,the value of $K_p$ 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 $R=0.0831 \, L \, bar \, K^{-1} \, mol^{-1}$]

$A$ schematic plot of $\ln K_{eq}$ versus inverse of temperature $(1/T)$ for a reaction is shown below. The reaction must be

In which of the following cases is $K_p$ less than $K_c$?