At 780 K and 10 atmosphere pressure the equilibrium constant for the reaction $2 A(g) \rightleftharpoons B(g)+C(g)$ is 3.52 . At the same temperature and 7.04 atmosphere pressure, the equilibrium constant for the same reaction is

Calculate the value of the equilibrium constant $\left(K_p\right)$ for the reaction of oxygen gas oxidising ammonia gas to nitric oxide and water vapour. The pressure of each gas at equilibrium is 0.5 atm .

For the formation of ammonia from its constituent elements ( 1 mole of $\mathrm{N}_2$ and 3 moles of $\mathrm{H}_2$ ) in a closed vessel of volume $V(\mathrm{~L})$, the value of $K_C$ is [units of $K_C=\mathrm{mol}^{-2} \mathrm{~L}^2$ ]

The $K_p$ value at equilibrium of $\mathrm{SO}_3$ formation reaction from $\mathrm{SO}_2(g)$ and $\mathrm{O}_2(g)$ is $5 \mathrm{~atm}^{-1}$. What is the equilibrium partial pressure of $\mathrm{O}_2$ if the equilibrium pressure of $\mathrm{SO}_2$ and $\mathrm{SO}_3$ are equal?