For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,the value of $K_c$ is $0.04$ at $250 \ ^oC$ in a $3 \ L$ vessel. If the concentration of $Cl_2$ at equilibrium is $0.15 \ M$,then the initial moles of $PCl_5$ will be ...........

The values of $K_{P_1}$ and $K_{P_2}$ for the reactions
$X \rightleftharpoons Y + Z$ --- $(1)$
$A \rightleftharpoons 2B$ --- $(2)$
are in the ratio of $9 : 1$. If the degree of dissociation of $X$ and $A$ is equal,then the total pressure at equilibrium for $(1)$ and $(2)$ are in the ratio:

In reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $B$ was $1.5$ times that of $[A]$,but at equilibrium,the concentrations of $A$ and $B$ became equal. The equilibrium constant for the reaction is:

The value of $K_{c} = 4.24$ at $800 \, K$ for the reaction,
$CO_{(g)} + H_{2}O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$
Calculate equilibrium concentrations of $CO_{2}$,$H_{2}$,$CO$ and $H_{2}O$ at $800 \, K$,if only $CO$ and $H_{2}O$ are present initially at concentrations of $0.10 \, M$ each.

Calculate the partial pressure of carbon monoxide from the following:
$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ ; $K_{p1} = 2$
$CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$ ; $K_{p2} = 8 \times 10^{-2}$

The partial pressures of an equilibrium mixture of $H_2$,$N_2$,and $NH_3$ are $2 \, atm$,$1 \, atm$,and $3 \, atm$ respectively. If the value of $K_P$ for the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$ at $725 \, K$ is $4.28 \times 10^{-5} \, atm^{-2}$,in which direction will the reaction proceed?