When one mole of $A$ and one mole of $B$ were heated in a one-litre flask at $T \ K$,$0.5 \ mole$ of $C$ was formed at equilibrium for the reaction $A + B \rightleftharpoons C + D$. The equilibrium constant,$K_C$,is:

For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$

Consider the following reaction in a $1 \ L$ closed vessel: $N_2 + 3H_2 \rightleftharpoons 2NH_3$. If all the species $N_2, H_2$ and $NH_3$ are $1 \ mol$ each at the beginning of the reaction and equilibrium is attained when unreacted $N_2$ is $0.7 \ mol$,what is the value of the equilibrium constant?

For the reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ at equilibrium,the partial pressures of $PCl_5, PCl_3$ and $Cl_2$ are $2 \ atm, 4 \ atm$ and $4 \ atm$ respectively. The value of $K_C$ at $27^{\circ}C$ is (approx):-

The equilibrium constant $K_p$ for the following reaction at $191\,^{\circ}C$ is $1.24$. What is the value of $K_c$? $B_{(s)} + \frac{3}{2}F_{2(g)} \rightleftharpoons BF_{3(g)}$

At $1000\, K$ and $2\, atm$ pressure,a gaseous mixture of $CO$ and $CO_{2}$ in equilibrium with solid carbon has $84\%$ $CO_{(g)}$ by mass. Calculate $K_{p}$ for the reaction: $C_{(s)} + CO_{2_{(g)}} \rightleftharpoons 2CO_{(g)}$ at this temperature.