If $0.5 \ mol$ of $H_2$ and $0.5 \ mol$ of $I_2$ are reacted in a $10 \ L$ vessel at $444 \ ^\circ C$,and the equilibrium constant $K_c$ at the same temperature is $49$,then the ratio of $[HI]$ to $[I_2]$ is .......

$2 \ mol$ $PCl_5$ is heated in a $4 \ L$ closed vessel at a definite temperature. At equilibrium,$55\%$ of $PCl_5$ remains undissociated. Find $K_c$. Reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$

$A$ sample of $HI_{(g)}$ is placed in a flask at a pressure of $0.2 \ atm$. At equilibrium,the partial pressure of $HI_{(g)}$ is $0.04 \ atm$. What is $K_{p}$ for the given equilibrium?
$2 HI_{(g)} \longleftrightarrow H_{2_{(g)}} + I_{2_{(g)}}$

For which of the following reactions is the relation $\log \frac{K_P}{K_C} + \log RT = 0$ correct?

In a system $A_{(s)} \rightleftharpoons 2B_{(g)} + 3C_{(g)},$ if the concentration of $C$ at equilibrium is increased by a factor of $2,$ it will cause the equilibrium concentration of $B$ to change to

$(i)$ $\frac{1}{2}N_{2(g)} + \frac{3}{2}H_{2(g)} \rightleftharpoons NH_{3(g)}$ at $298 \ K$ has $\Delta G^{\Theta} = -16.5 \ kJ \ mol^{-1}$. Find $K_p$.
$(ii)$ At $298 \ K$,for $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$,calculate $K_p$ and $\Delta G^{\Theta}$.