In the thermal dissociation of $PCl_5$,the total pressure in the gaseous equilibrium mixture is $1.0 \ atm$ when half of $PCl_5$ is found to dissociate. The equilibrium constant of the reaction $(K_p)$ in atmosphere is

At $527 \ ^oC$,the reaction given below has $K_c = 4$.
$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$
What is the $K_P$ for the following reaction?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

Pure $PCl_5$ is introduced into an evacuated chamber and comes to equilibrium at $247\, ^oC$ and $2.0\ atm$. The equilibrium gaseous mixture contains $40\%$ chlorine by volume. Calculate $K_p$ at $247\, ^oC$ for the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ in $atm$.

For the reaction: $H_{2(g)} + CO_{2(g)} \rightleftharpoons CO_{(g)} + H_2O_{(g)}$,if the initial concentration of $[H_2] = [CO_2] = 1 \ M$ and $x \ mol/L$ of hydrogen is consumed at equilibrium,the correct expression for $K_c$ is:

The equilibrium constant $(K_P)$ for the reaction $2SO_2 + O_2 \rightleftharpoons 2SO_3$ at $1000 \ K$ is $3.5$. The partial pressure of oxygen gas to give equal mole of $SO_2$ and $SO_3$ is $... \ atm$.

For the given equilibrium reaction,$2 A(g) \rightleftharpoons 2 B(g) + C(g)$,the equilibrium constant $(K_c)$ at $1000 \ K$ is $4 \times 10^{-4}$. Calculate $K_p$ for the reaction at $800 \ K$ temperature.