For the reversible reaction $2HI_{(g)} \rightleftharpoons H_{2(g)} + I_{2(g)}$, the unit of the equilibrium constant $K_c$ is:

When $4 \ mol$ of $A$ is mixed with $4 \ mol$ of $B$,$2 \ mol$ of $C$ is formed at equilibrium. For the reaction $A + B \rightleftharpoons C + D$,the equilibrium constant is:

At a definite temperature,the equilibrium constant $K_{c}$ is given by the following equation: $K_{c} = \frac{[I_{2}][H_{5}IO_{6}]^{5}}{[IO_{3}^{-}]^{7}[H_{2}O]^{9}[H^{+}]^{7}}$. Write the balanced chemical equilibrium equation.

The equilibrium constant for the reaction $PCl_{5(g)} \to PCl_{3(g)} + Cl_{2(g)}$ is $16$. If the volume of the container is reduced to one half its original volume,the value of $K_p$ for the reaction at the same temperature will be

The reaction,$CO_{(g)} + 3H_{2(g)} \longleftrightarrow CH_{4(g)} + H_{2}O_{(g)}$ is at equilibrium at $1300 \, K$ in a $1 \, L$ flask. It also contains $0.30 \, mol$ of $CO$,$0.10 \, mol$ of $H_{2}$,and $0.02 \, mol$ of $H_{2}O$ and an unknown amount of $CH_{4}$ in the flask. Determine the concentration of $CH_{4}$ in the mixture. The equilibrium constant,$K_{c}$ for the reaction at the given temperature is $3.90$.

On a given condition,the equilibrium concentrations of $HI$,$H_2$,and $I_2$ are $0.80 \ mol/L$,$0.10 \ mol/L$,and $0.10 \ mol/L$ respectively. The equilibrium constant for the reaction $H_2 + I_2 \rightleftharpoons 2HI$ will be: