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 equilibrium constant $(K_p)$ for the formation of ammonia from its constituent elements at $27^{\circ} C$ is $1.2 \times 10^{-4}$ and at $127^{\circ} C$ is $0.60 \times 10^{-4}$. Calculate the mean heat of formation of ammonia per mole in this temperature range. (in $cal$)

For the reaction $2A_{(g)} \rightleftharpoons B_{(g)} + 3C_{(g)}$,at a given temperature $K_c = 16$,what must be the volume of the flask if a mixture of $2 \ mol$ each of $A, B, C$ exists at equilibrium?

For the reversible reaction $A + B \rightleftharpoons C + D$,the equilibrium concentrations of $C$ and $D$ are $0.8 \ mol/L$ each. If the initial concentrations of $A$ and $B$ were $1 \ mol/L$ each,calculate the equilibrium constant $K_c$.

For the reaction,$2A_{(g)} \rightleftharpoons 3C_{(g)} + D_{(g)}$,the value of $K_c$ will be equal to:

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