For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $\frac{K_c}{K_p}$ is:

For the reaction $CO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons CO_{2(g)}$,the value of $K_P/K_C$ is

At a definite temperature and $3 \ atm$ pressure,$75\%$ of $PCl_5$ decomposes into $PCl_3$ and $Cl_2$. Find $K_p$ for the reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ (in $atm$)

Find out the value of $K_C$ for the following reaction from the value of $K_P$:
$2NOCl_{(g)} \rightleftharpoons 2NO_{(g)} + Cl_{2(g)}$
Given: $K_P = 8 \times 10^{12} \ atm$ at $500 \ K$,use $R = 0.08 \ L \ atm \ mol^{-1} \ K^{-1}$.

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,$1 mol$ of $PCl_5$ is taken at $5 atm$ pressure. If $50\%$ of $PCl_5$ dissociates at equilibrium,calculate $K_p$.

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,the equilibrium constant $K_p = 41$ at $400 \ K$. Calculate $K_c$ for the following reactions at $400 \ K$:
$(a)$ $2N_{2(g)} + 6H_{2(g)} \rightleftharpoons 4NH_{3(g)}$
$(b)$ $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$
$(c)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$