What is the unit of $K_p$ for the reaction?
$CS_{2(g)} + 4H_{2(g)} \to CH_{4(g)} + 2H_2S_{(g)}$

For the reaction $NH_4COONH_2(s) \rightleftharpoons 2NH_3(g) + CO_2(g)$,the equilibrium pressure is $3 \ atm$. Calculate $K_p$.

For the reaction $A_{(g)} \rightleftharpoons 2 B_{(g)}$,the backward reaction rate constant is higher than the forward reaction rate constant by a factor of $2500$,at $1000 \ K$. [Given : $R = 0.0831 \ L \ atm \ mol^{-1} \ K^{-1}$] $K_p$ for the reaction at $1000 \ K$ 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:

$A$ sample of $HI_{(g)}$ is placed in a flask at a pressure of $0.2 \ atm$. At equilibrium,the partial pressure of $HI_{(g)}$ is $0.04 \ atm$. What is $K_{p}$ for the given equilibrium?
$2 HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$

The equilibrium $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ shows that $K_P$ (in $atm$) is double the value of $K_C$ (in $mol/L$) at a particular temperature $T$. Then,$T$ is $...... \ K$.