At $500 \ K$,for the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the $K_p$ is $0.036 \ atm^{-2}$. What is its $K_C$ in $L^2 \ mol^{-2}$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

For the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_p$ at $1000 \ K$ is $0.05 \ atm$. The value of $K_c$ in terms of $R$ will be:

In which of the following reactions is $K_p > K_c$ at $10 \ K$ temperature?

For the reaction $H_{2(g)} + CO_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$,if the reaction is started with $1 \ mol$ of $H_2$ and $CO_2$ each,and $x \ mol/L$ of $H_2$ is consumed at equilibrium,then the correct expression for $K_p$ will be ........

$XY_2$ dissociates as $XY_{2(g)} \rightleftharpoons XY_{(g)} + Y_{(g)}$. When the initial pressure of $XY_2$ is $600 \ mm \ Hg$,the total equilibrium pressure is $800 \ mm \ Hg$. Calculate $K_p$ for the reaction,assuming the volume of the system remains unchanged.

For which of the following reactions is the relation $\frac{K_p}{K_c} + \log(RT) = 0$ correct?