$2 \ mol$ of $PCl_5$ is heated in a closed vessel of $2 \ L$ capacity. When equilibrium is attained,$PCl_5$ is $40\%$ dissociated. The equilibrium constant $K_c$ for the reaction will be ........... $mol/L$.

For the following gas phase equilibrium reaction at constant temperature,$NH_{3(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{3}{2} H_{2(g)}$. If the total pressure is $\sqrt{3} \ atm$ and the pressure equilibrium constant $(K_p)$ is $9 \ atm$,then the degree of dissociation is given as $(x \times 10^{-2})^{-1/2}$. The value of $x$ is . . . . . . (Nearest integer)

The value of $K_{p}$ for the reaction,$CO_{2(g)} + C_{(s)} \rightleftharpoons 2CO_{(g)}$ is $3.0$ at $1000 \ K$. If initially $P_{CO_{2}} = 0.48 \ bar$ and $P_{CO} = 0 \ bar$ and pure graphite is present,calculate the equilibrium partial pressures of $CO$ and $CO_{2}$.

For the chemical reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,$\Delta H^o$ of reaction can be determined from which one of the following plots?

The value of $\log \ K$ for the reaction $A \rightleftharpoons B$ at $298 \ K$ is (Nearest integer).
Given: $\Delta H^{\circ} = -54.07 \ kJ \ mol^{-1}$
$\Delta S^{\circ} = 10 \ J \ K^{-1} \ mol^{-1}$
(Take $2.303 \times 8.314 \times 298 = 5705$)

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ at $300 \, ^\circ C$,the value of $K_c$ is $0.65$. If $R = 0.082 \, L \cdot atm \cdot K^{-1} \cdot mol^{-1}$,then the value of $K_p$ will be: