For the reaction $ZnCO_{3(s)} \rightleftharpoons ZnO_{(s)} + CO_{2(g)}$,the expression for the equilibrium constant in terms of partial pressure $(K_p)$ is .............

$K_{p} = 0.04 \ atm$ at $899 \ K$ for the equilibrium shown below. What is the equilibrium pressure of $C_{2}H_{6}$ when it is placed in a flask at $4.0 \ atm$ pressure and allowed to come to equilibrium?
$C_{2}H_{6(g)} \longleftrightarrow C_{2}H_{4(g)} + H_{2(g)}$

Which of the following relations is correct for $k_f$ and $k_b$ in an equilibrium process that contains equal moles of reactants and products?

At $1050 \ K$,for the chemical reaction $FeO_{(s)} + CO_{(g)} \rightleftharpoons Fe_{(s)} + CO_{2_{(g)}}$; $K_p = 0.25$. What are the equilibrium partial pressures of $CO_{(g)}$ and $CO_{2_{(g)}}$ at $1050 \ K$,if the initial partial pressures are: $P_{CO_{(g)}} = 1.6 \ atm$ and $P_{CO_{2_{(g)}}} = 0.8 \ atm$?

In which of the following equilibrium $K_c$ and $K_p$ are not equal?

The equilibrium constant of $NH_4COONH_2$ in a closed vessel at $400 \ K$ temperature is $600 \ bar^3$. What will be the total pressure at equilibrium (in $bar$)?
$NH_4COONH_{2(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$