For the following reaction in gaseous phase $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,$K_p/K_c$ is

The partial pressures of $CH_3OH$,$CO$ and $H_2$ in the equilibrium mixture for the reaction $CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g)$ at $427 \ ^oC$ are $2.0 \ atm$,$1.0 \ atm$ and $0.1 \ atm$ respectively. The value of $K_P$ for the decomposition of $CH_3OH$ to $CO$ and $H_2$ is:

$A + B \rightleftharpoons C + D$. If the final equilibrium concentrations of $A$ and $B$ are equal,and the equilibrium concentration of $D$ is twice that of $A$,what is the equilibrium constant $(K_c)$ of the reaction?

An amount of solid $NH_4HS$ is placed in a flask already containing ammonia gas at a certain temperature and $0.50 \ atm$ pressure. Ammonium hydrogen sulphide decomposes to yield $NH_3$ and $H_2S$ gases in the flask. When the decomposition reaction reaches equilibrium,the total pressure in the flask rises to $0.84 \ atm$. The equilibrium constant for $NH_4HS$ decomposition at this temperature is

If ${K_c}$ is the equilibrium constant for the formation of $NH_3$,the dissociation constant of ammonia under the same temperature will be

For the equilibrium reaction $CO + 2H_2 \rightleftharpoons CH_3OH$ at $427 \, ^\circ C$,the partial pressures of $CH_3OH$,$CO$,and $H_2$ are $2.0 \, atm$,$1.0 \, atm$,and $0.1 \, atm$ respectively. What is the value of $K_P$ for the decomposition of $CH_3OH$?