164021 If \(8 \mathrm{~g} \mathrm{~mol}\) of \(\mathrm{PCl}_5\) heated in a closed vessel of 10 L capacity and \(25 \%\) of it dissociates into \(\mathrm{PCl}_3\) and \(\mathrm{Cl}_2\) at the equilibrium then value of \(\mathrm{Kp}\) will be equal to: ( \(P\) is total pressure)

164022 In the reaction \(2 \mathrm{P}(\mathrm{g})+\mathrm{Q}(\mathrm{g}) \rightleftharpoons 3 \mathrm{R}(\mathrm{g})+\mathrm{S}(\mathrm{g})\). If 2 mol each of \(P\) and \(Q\) taken initially in a 1 L flask. At equilibrium which is true:

164023 'a' mol of \(\mathrm{PCl}_5\), undergoes, thermal dissociation as: \(\mathrm{PCl}_5 \rightleftharpoons \mathrm{PCl}_3+\mathrm{Cl}_2\), the mole fraction of \(\mathrm{PCl}_3\) at equilibrium is \(\mathbf{0 . 2 5}\) and the total pressure is \(\mathbf{2 . 0}\) atm. The partial pressure of \(\mathrm{Cl}_2\) at equilibrium is:

164024 Evaluate \(K_P\) for the reaction: \(H_2+I_2 \rightleftharpoons 2 H\). If 2 moles each of \(\mathrm{H}_2\) and \(\mathrm{I}_2\) are taken initially. The equilibrium moles of \(\mathrm{HI}\) are 2.

164021 If \(8 \mathrm{~g} \mathrm{~mol}\) of \(\mathrm{PCl}_5\) heated in a closed vessel of 10 L capacity and \(25 \%\) of it dissociates into \(\mathrm{PCl}_3\) and \(\mathrm{Cl}_2\) at the equilibrium then value of \(\mathrm{Kp}\) will be equal to: ( \(P\) is total pressure)

164022 In the reaction \(2 \mathrm{P}(\mathrm{g})+\mathrm{Q}(\mathrm{g}) \rightleftharpoons 3 \mathrm{R}(\mathrm{g})+\mathrm{S}(\mathrm{g})\). If 2 mol each of \(P\) and \(Q\) taken initially in a 1 L flask. At equilibrium which is true:

164023 'a' mol of \(\mathrm{PCl}_5\), undergoes, thermal dissociation as: \(\mathrm{PCl}_5 \rightleftharpoons \mathrm{PCl}_3+\mathrm{Cl}_2\), the mole fraction of \(\mathrm{PCl}_3\) at equilibrium is \(\mathbf{0 . 2 5}\) and the total pressure is \(\mathbf{2 . 0}\) atm. The partial pressure of \(\mathrm{Cl}_2\) at equilibrium is:

164024 Evaluate \(K_P\) for the reaction: \(H_2+I_2 \rightleftharpoons 2 H\). If 2 moles each of \(\mathrm{H}_2\) and \(\mathrm{I}_2\) are taken initially. The equilibrium moles of \(\mathrm{HI}\) are 2.

164021 If \(8 \mathrm{~g} \mathrm{~mol}\) of \(\mathrm{PCl}_5\) heated in a closed vessel of 10 L capacity and \(25 \%\) of it dissociates into \(\mathrm{PCl}_3\) and \(\mathrm{Cl}_2\) at the equilibrium then value of \(\mathrm{Kp}\) will be equal to: ( \(P\) is total pressure)

164022 In the reaction \(2 \mathrm{P}(\mathrm{g})+\mathrm{Q}(\mathrm{g}) \rightleftharpoons 3 \mathrm{R}(\mathrm{g})+\mathrm{S}(\mathrm{g})\). If 2 mol each of \(P\) and \(Q\) taken initially in a 1 L flask. At equilibrium which is true:

164023 'a' mol of \(\mathrm{PCl}_5\), undergoes, thermal dissociation as: \(\mathrm{PCl}_5 \rightleftharpoons \mathrm{PCl}_3+\mathrm{Cl}_2\), the mole fraction of \(\mathrm{PCl}_3\) at equilibrium is \(\mathbf{0 . 2 5}\) and the total pressure is \(\mathbf{2 . 0}\) atm. The partial pressure of \(\mathrm{Cl}_2\) at equilibrium is:

164024 Evaluate \(K_P\) for the reaction: \(H_2+I_2 \rightleftharpoons 2 H\). If 2 moles each of \(\mathrm{H}_2\) and \(\mathrm{I}_2\) are taken initially. The equilibrium moles of \(\mathrm{HI}\) are 2.

164021 If \(8 \mathrm{~g} \mathrm{~mol}\) of \(\mathrm{PCl}_5\) heated in a closed vessel of 10 L capacity and \(25 \%\) of it dissociates into \(\mathrm{PCl}_3\) and \(\mathrm{Cl}_2\) at the equilibrium then value of \(\mathrm{Kp}\) will be equal to: ( \(P\) is total pressure)

164022 In the reaction \(2 \mathrm{P}(\mathrm{g})+\mathrm{Q}(\mathrm{g}) \rightleftharpoons 3 \mathrm{R}(\mathrm{g})+\mathrm{S}(\mathrm{g})\). If 2 mol each of \(P\) and \(Q\) taken initially in a 1 L flask. At equilibrium which is true:

164023 'a' mol of \(\mathrm{PCl}_5\), undergoes, thermal dissociation as: \(\mathrm{PCl}_5 \rightleftharpoons \mathrm{PCl}_3+\mathrm{Cl}_2\), the mole fraction of \(\mathrm{PCl}_3\) at equilibrium is \(\mathbf{0 . 2 5}\) and the total pressure is \(\mathbf{2 . 0}\) atm. The partial pressure of \(\mathrm{Cl}_2\) at equilibrium is:

164024 Evaluate \(K_P\) for the reaction: \(H_2+I_2 \rightleftharpoons 2 H\). If 2 moles each of \(\mathrm{H}_2\) and \(\mathrm{I}_2\) are taken initially. The equilibrium moles of \(\mathrm{HI}\) are 2.