In a chemical reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $B$ was $1.5$ times of $A$ but the equilibrium concentrations of $A$ and $B$ were found to be equal. The equilibrium constant $(K)$ for the aforesaid chemical reaction is

For the gas phase reaction; $C_2H_{4(g)} + H_{2(g)} \rightleftharpoons C_2H_{6(g)}$,$\Delta H = -32.7 \ kcal$ carried out in a vessel,the equilibrium concentration of $C_2H_4$ can be increased by:

$A$ plot of $\ln K$ against $\frac{1}{T}$ ($x$-axis) is expected to be a straight line,with intercept on $Y$-axis equal to

The equilibrium constant for the following reaction is $1.6 \times 10^{5}$ at $1024 \, K$:
$H_{2(g)} + Br_{2(g)} \longleftrightarrow 2HBr_{(g)}$
Find the equilibrium pressure of all gases if $10.0 \, bar$ of $HBr$ is introduced into a sealed container at $1024 \, K$.

For the equilibrium $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$,the partial pressures of $SO_2$,$O_2$,and $SO_3$ are $0.662 \ atm$,$0.101 \ atm$,and $0.331 \ atm$ respectively. If the equilibrium concentrations of $SO_2$ and $SO_3$ are made equal,the partial pressure of $O_2$ will be ..... $atm$.

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