For the following reaction in gaseous phase $CO + 1/2 O_2 \to CO_2$,the ratio $K_p/K_c$ is:

The equilibrium concentrations of $X$,$Y$,and $YX_2$ are $4 \ mol/L$,$2 \ mol/L$,and $2 \ mol/L$ respectively for the equilibrium $2X + Y \rightleftharpoons YX_2$. The value of $K_c$ is:

The reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ is started by taking $0.8 \ mol$ of $N_2O_4$ in a $1 \ L$ flask. If the equilibrium constant at $298 \ K$ is $0.00466 \ M$,the equilibrium concentration of $NO_2$ will be ........... $M$.

$9.2 \ g$ of $N_2O_{4(g)}$ is taken in a $1 \ L$ closed vessel and heated until the following equilibrium is attained:
${N_2}{O_{4(g)}} \rightleftharpoons 2N{O_{2(g)}}$
If $50\%$ of $N_2O_{4(g)}$ dissociates at equilibrium,what will be the equilibrium constant (in $mol \ L^{-1}$)? (Mol. wt. of $N_2O_4 = 92$)

At $1000 \ K$,a vessel contains $CO_2$ at a pressure of $0.5 \ atm$. Some $CO_2$ is converted into $CO$ by the addition of graphite. If the total pressure at equilibrium is $0.8 \ atm$,what is the value of $K_p$ in $atm$?

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)