319481 The total vapor pressure of a 4 mole% solution of \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) in water at 293 K is 50 torr. The vapor pressure of pure water is 17 torr at this temperature. Applying Henry's law i.e., Solubility \({\rm{ = }}{{\rm{K}}_{\rm{H}}}{\rm{ \times }}\) Pressure and Raoult's law, calculate the total vapour pressure for a 5 mole % solution.
319482 The solubility of \({{\rm{N}}_{\rm{2}}}\) in water at 300 K and 500 torr partial pressure is \({\rm{0}}{\rm{.01g}}{{\rm{L}}^{{\rm{ - 1}}}}\). The solubility \(\left( {{\rm{in}}{\mkern 1mu} {\mkern 1mu} {\rm{g}}{{\rm{L}}^{{\rm{ - 1}}}}} \right)\) at 750 torr partial pressure is :
319483 At \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\), the vapour pressure of pure liquid ‘A’ is 520 mm Hg and that of pure liquid ‘B’ is 1000 mm Hg. If a mixture of solution of ‘A’ and ‘B’ boils at \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\) and 1 atm pressure, the amount of ‘A’ in the mixture is (1 atm = 760 mm Hg)
319481 The total vapor pressure of a 4 mole% solution of \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) in water at 293 K is 50 torr. The vapor pressure of pure water is 17 torr at this temperature. Applying Henry's law i.e., Solubility \({\rm{ = }}{{\rm{K}}_{\rm{H}}}{\rm{ \times }}\) Pressure and Raoult's law, calculate the total vapour pressure for a 5 mole % solution.
319482 The solubility of \({{\rm{N}}_{\rm{2}}}\) in water at 300 K and 500 torr partial pressure is \({\rm{0}}{\rm{.01g}}{{\rm{L}}^{{\rm{ - 1}}}}\). The solubility \(\left( {{\rm{in}}{\mkern 1mu} {\mkern 1mu} {\rm{g}}{{\rm{L}}^{{\rm{ - 1}}}}} \right)\) at 750 torr partial pressure is :
319483 At \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\), the vapour pressure of pure liquid ‘A’ is 520 mm Hg and that of pure liquid ‘B’ is 1000 mm Hg. If a mixture of solution of ‘A’ and ‘B’ boils at \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\) and 1 atm pressure, the amount of ‘A’ in the mixture is (1 atm = 760 mm Hg)
319481 The total vapor pressure of a 4 mole% solution of \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) in water at 293 K is 50 torr. The vapor pressure of pure water is 17 torr at this temperature. Applying Henry's law i.e., Solubility \({\rm{ = }}{{\rm{K}}_{\rm{H}}}{\rm{ \times }}\) Pressure and Raoult's law, calculate the total vapour pressure for a 5 mole % solution.
319482 The solubility of \({{\rm{N}}_{\rm{2}}}\) in water at 300 K and 500 torr partial pressure is \({\rm{0}}{\rm{.01g}}{{\rm{L}}^{{\rm{ - 1}}}}\). The solubility \(\left( {{\rm{in}}{\mkern 1mu} {\mkern 1mu} {\rm{g}}{{\rm{L}}^{{\rm{ - 1}}}}} \right)\) at 750 torr partial pressure is :
319483 At \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\), the vapour pressure of pure liquid ‘A’ is 520 mm Hg and that of pure liquid ‘B’ is 1000 mm Hg. If a mixture of solution of ‘A’ and ‘B’ boils at \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\) and 1 atm pressure, the amount of ‘A’ in the mixture is (1 atm = 760 mm Hg)
319481 The total vapor pressure of a 4 mole% solution of \({\rm{N}}{{\rm{H}}_{\rm{3}}}\) in water at 293 K is 50 torr. The vapor pressure of pure water is 17 torr at this temperature. Applying Henry's law i.e., Solubility \({\rm{ = }}{{\rm{K}}_{\rm{H}}}{\rm{ \times }}\) Pressure and Raoult's law, calculate the total vapour pressure for a 5 mole % solution.
319482 The solubility of \({{\rm{N}}_{\rm{2}}}\) in water at 300 K and 500 torr partial pressure is \({\rm{0}}{\rm{.01g}}{{\rm{L}}^{{\rm{ - 1}}}}\). The solubility \(\left( {{\rm{in}}{\mkern 1mu} {\mkern 1mu} {\rm{g}}{{\rm{L}}^{{\rm{ - 1}}}}} \right)\) at 750 torr partial pressure is :
319483 At \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\), the vapour pressure of pure liquid ‘A’ is 520 mm Hg and that of pure liquid ‘B’ is 1000 mm Hg. If a mixture of solution of ‘A’ and ‘B’ boils at \({\rm{8}}{{\rm{0}}^{\rm{^\circ }}}{\rm{C}}\) and 1 atm pressure, the amount of ‘A’ in the mixture is (1 atm = 760 mm Hg)