For the reaction $2P_{(g)} + Q_{(g)} \rightleftharpoons R_{(g)} + S_{(g)}$; $K_C = 10^{12}$. If the initial moles of $P, Q, R, S$ are $2, 1, 7$ and $3$ moles respectively in a $1 \ L$ vessel,find the equilibrium concentration of $P$.

The distribution law is applied for the distribution of a solute between which of the following pairs of solvents?

For the esterification reaction $CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5(l)} + H_2O_{(l)}$,the equilibrium constant $K_c$ is $4$. If $4 \ mol$ of each acid and alcohol are taken initially,what will be the concentration of the acid at equilibrium?

At $T(K)$,the $K_p$ for the reaction $A_2B_{6(g)} \rightleftharpoons A_2B_{4(g)} + B_{2(g)}$ is $0.04 \text{ atm}$. The equilibrium pressure (in $\text{atm}$) of $A_2B_{6(g)}$ when it is placed in a flask at $4 \text{ atm}$ pressure and allowed to come to equilibrium is:

The equilibrium constants $K_{p1}$ and $K_{p2}$ for the reactions $X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q$ respectively are in the ratio of $1 : 9$. If the degree of dissociation of $X$ and $Z$ be equal,then the ratio of total pressures at these equilibria is:

$A$ reaction mixture containing $H_2, N_2$ and $NH_3$ has partial pressures of $2 \ atm, 1 \ atm$ and $3 \ atm$ respectively at $725 \ K.$ If the value of $K_P$ for the reaction,$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$ is $4.28 \times 10^{-5} \ atm^{-2}$ at $725 \ K,$ in which direction will the net reaction proceed?