163821 If \(\mathbf{P}_0\) and \(\mathbf{P}_{\mathrm{s}}\) are the vapour pressure of solvent and its solution respectively. \(\mathrm{N}_1\) and \(\mathrm{N}_2\) are the mole fraction of solvent and solute respectively then:

163822 The vapour pressure of a dilute aqueous solution of Glucose is \(750 \mathrm{~mm} \mathrm{Hg}\) at \(373 \mathrm{~K}\). The mole fraction of solute is:

163823 The vapour pressure of pure \(A\) is 10 torr. At the same temperature, when \(1 \mathrm{~g}\) of \(B\) is dissolved in \(20 \mathrm{gm}\) of \(\mathrm{A}\), its vapour pressure is reduced to 9.0 torr. If the molecular mass of \(A\) is \(200 \mathrm{amu}\), then the molecular mass of \(B\) is:

163824 The boiling point of an aqueous solution of a non volatile solute is \(100.15^{\circ} \mathrm{C}\). What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The values of \(K_b\) and \(K_f\) for water are 0.512 and \(1.86 \mathrm{~K} \mathrm{molality}^{-1}\) :

163821 If \(\mathbf{P}_0\) and \(\mathbf{P}_{\mathrm{s}}\) are the vapour pressure of solvent and its solution respectively. \(\mathrm{N}_1\) and \(\mathrm{N}_2\) are the mole fraction of solvent and solute respectively then:

163822 The vapour pressure of a dilute aqueous solution of Glucose is \(750 \mathrm{~mm} \mathrm{Hg}\) at \(373 \mathrm{~K}\). The mole fraction of solute is:

163823 The vapour pressure of pure \(A\) is 10 torr. At the same temperature, when \(1 \mathrm{~g}\) of \(B\) is dissolved in \(20 \mathrm{gm}\) of \(\mathrm{A}\), its vapour pressure is reduced to 9.0 torr. If the molecular mass of \(A\) is \(200 \mathrm{amu}\), then the molecular mass of \(B\) is:

163824 The boiling point of an aqueous solution of a non volatile solute is \(100.15^{\circ} \mathrm{C}\). What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The values of \(K_b\) and \(K_f\) for water are 0.512 and \(1.86 \mathrm{~K} \mathrm{molality}^{-1}\) :

163821 If \(\mathbf{P}_0\) and \(\mathbf{P}_{\mathrm{s}}\) are the vapour pressure of solvent and its solution respectively. \(\mathrm{N}_1\) and \(\mathrm{N}_2\) are the mole fraction of solvent and solute respectively then:

163822 The vapour pressure of a dilute aqueous solution of Glucose is \(750 \mathrm{~mm} \mathrm{Hg}\) at \(373 \mathrm{~K}\). The mole fraction of solute is:

163823 The vapour pressure of pure \(A\) is 10 torr. At the same temperature, when \(1 \mathrm{~g}\) of \(B\) is dissolved in \(20 \mathrm{gm}\) of \(\mathrm{A}\), its vapour pressure is reduced to 9.0 torr. If the molecular mass of \(A\) is \(200 \mathrm{amu}\), then the molecular mass of \(B\) is:

163824 The boiling point of an aqueous solution of a non volatile solute is \(100.15^{\circ} \mathrm{C}\). What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The values of \(K_b\) and \(K_f\) for water are 0.512 and \(1.86 \mathrm{~K} \mathrm{molality}^{-1}\) :

163821 If \(\mathbf{P}_0\) and \(\mathbf{P}_{\mathrm{s}}\) are the vapour pressure of solvent and its solution respectively. \(\mathrm{N}_1\) and \(\mathrm{N}_2\) are the mole fraction of solvent and solute respectively then:

163822 The vapour pressure of a dilute aqueous solution of Glucose is \(750 \mathrm{~mm} \mathrm{Hg}\) at \(373 \mathrm{~K}\). The mole fraction of solute is:

163823 The vapour pressure of pure \(A\) is 10 torr. At the same temperature, when \(1 \mathrm{~g}\) of \(B\) is dissolved in \(20 \mathrm{gm}\) of \(\mathrm{A}\), its vapour pressure is reduced to 9.0 torr. If the molecular mass of \(A\) is \(200 \mathrm{amu}\), then the molecular mass of \(B\) is:

163824 The boiling point of an aqueous solution of a non volatile solute is \(100.15^{\circ} \mathrm{C}\). What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The values of \(K_b\) and \(K_f\) for water are 0.512 and \(1.86 \mathrm{~K} \mathrm{molality}^{-1}\) :