277348 Molar enthalpy change for melting of ice is 6 $\mathrm{kJ} / \mathrm{mol}$. Then the internal energy change (in $\mathrm{kJ} / \mathrm{mol}$ ) when 1 mole of water is converted into ice at $1 \mathrm{~atm}$ at $0^{\circ} \mathrm{C}$ is

277349 $18 \mathrm{~g}$ of glucose is dissolved in $90 \mathrm{~g}$ of water. The relative lowering of vapour pressure of the solution is equal to :

277350 The vapour pressure of acetone at $20^{\circ} \mathrm{C}$ is 185 torr. When $1.2 \mathrm{~g}$ of a non-volatile substance was dissolved in $100 \mathrm{~g}$ of acetone at $20^{\circ} \mathrm{C}$, its vapour pressure was 183 torr. The molar mass ( $\mathrm{g} \mathrm{mol}^{-}$ 1 ) of the substance is

277351 The vapour pressure of pure liquid solvent $A$ is 0.80 bar. When a non-volatile substance $B$ is added to the solvent, its vapor pressure drops to 0.60 bar. What is the mole fraction of component $B$ in the solution?

277352 To observe an elevation of boiling point of $0.05^{\circ} \mathrm{C}$, the amount of a solute $(\mathrm{mol} . \mathrm{wt}=100)$ to be added to $100 \mathrm{~g}$ of water $\left(K_{b}=0.5\right)$ is

277348 Molar enthalpy change for melting of ice is 6 $\mathrm{kJ} / \mathrm{mol}$. Then the internal energy change (in $\mathrm{kJ} / \mathrm{mol}$ ) when 1 mole of water is converted into ice at $1 \mathrm{~atm}$ at $0^{\circ} \mathrm{C}$ is

277349 $18 \mathrm{~g}$ of glucose is dissolved in $90 \mathrm{~g}$ of water. The relative lowering of vapour pressure of the solution is equal to :

277350 The vapour pressure of acetone at $20^{\circ} \mathrm{C}$ is 185 torr. When $1.2 \mathrm{~g}$ of a non-volatile substance was dissolved in $100 \mathrm{~g}$ of acetone at $20^{\circ} \mathrm{C}$, its vapour pressure was 183 torr. The molar mass ( $\mathrm{g} \mathrm{mol}^{-}$ 1 ) of the substance is

277351 The vapour pressure of pure liquid solvent $A$ is 0.80 bar. When a non-volatile substance $B$ is added to the solvent, its vapor pressure drops to 0.60 bar. What is the mole fraction of component $B$ in the solution?

277352 To observe an elevation of boiling point of $0.05^{\circ} \mathrm{C}$, the amount of a solute $(\mathrm{mol} . \mathrm{wt}=100)$ to be added to $100 \mathrm{~g}$ of water $\left(K_{b}=0.5\right)$ is

277348 Molar enthalpy change for melting of ice is 6 $\mathrm{kJ} / \mathrm{mol}$. Then the internal energy change (in $\mathrm{kJ} / \mathrm{mol}$ ) when 1 mole of water is converted into ice at $1 \mathrm{~atm}$ at $0^{\circ} \mathrm{C}$ is

277349 $18 \mathrm{~g}$ of glucose is dissolved in $90 \mathrm{~g}$ of water. The relative lowering of vapour pressure of the solution is equal to :

277350 The vapour pressure of acetone at $20^{\circ} \mathrm{C}$ is 185 torr. When $1.2 \mathrm{~g}$ of a non-volatile substance was dissolved in $100 \mathrm{~g}$ of acetone at $20^{\circ} \mathrm{C}$, its vapour pressure was 183 torr. The molar mass ( $\mathrm{g} \mathrm{mol}^{-}$ 1 ) of the substance is

277351 The vapour pressure of pure liquid solvent $A$ is 0.80 bar. When a non-volatile substance $B$ is added to the solvent, its vapor pressure drops to 0.60 bar. What is the mole fraction of component $B$ in the solution?

277352 To observe an elevation of boiling point of $0.05^{\circ} \mathrm{C}$, the amount of a solute $(\mathrm{mol} . \mathrm{wt}=100)$ to be added to $100 \mathrm{~g}$ of water $\left(K_{b}=0.5\right)$ is

277348 Molar enthalpy change for melting of ice is 6 $\mathrm{kJ} / \mathrm{mol}$. Then the internal energy change (in $\mathrm{kJ} / \mathrm{mol}$ ) when 1 mole of water is converted into ice at $1 \mathrm{~atm}$ at $0^{\circ} \mathrm{C}$ is

277349 $18 \mathrm{~g}$ of glucose is dissolved in $90 \mathrm{~g}$ of water. The relative lowering of vapour pressure of the solution is equal to :

277350 The vapour pressure of acetone at $20^{\circ} \mathrm{C}$ is 185 torr. When $1.2 \mathrm{~g}$ of a non-volatile substance was dissolved in $100 \mathrm{~g}$ of acetone at $20^{\circ} \mathrm{C}$, its vapour pressure was 183 torr. The molar mass ( $\mathrm{g} \mathrm{mol}^{-}$ 1 ) of the substance is

277351 The vapour pressure of pure liquid solvent $A$ is 0.80 bar. When a non-volatile substance $B$ is added to the solvent, its vapor pressure drops to 0.60 bar. What is the mole fraction of component $B$ in the solution?

277352 To observe an elevation of boiling point of $0.05^{\circ} \mathrm{C}$, the amount of a solute $(\mathrm{mol} . \mathrm{wt}=100)$ to be added to $100 \mathrm{~g}$ of water $\left(K_{b}=0.5\right)$ is

277348 Molar enthalpy change for melting of ice is 6 $\mathrm{kJ} / \mathrm{mol}$. Then the internal energy change (in $\mathrm{kJ} / \mathrm{mol}$ ) when 1 mole of water is converted into ice at $1 \mathrm{~atm}$ at $0^{\circ} \mathrm{C}$ is

277349 $18 \mathrm{~g}$ of glucose is dissolved in $90 \mathrm{~g}$ of water. The relative lowering of vapour pressure of the solution is equal to :

277350 The vapour pressure of acetone at $20^{\circ} \mathrm{C}$ is 185 torr. When $1.2 \mathrm{~g}$ of a non-volatile substance was dissolved in $100 \mathrm{~g}$ of acetone at $20^{\circ} \mathrm{C}$, its vapour pressure was 183 torr. The molar mass ( $\mathrm{g} \mathrm{mol}^{-}$ 1 ) of the substance is

277351 The vapour pressure of pure liquid solvent $A$ is 0.80 bar. When a non-volatile substance $B$ is added to the solvent, its vapor pressure drops to 0.60 bar. What is the mole fraction of component $B$ in the solution?

277352 To observe an elevation of boiling point of $0.05^{\circ} \mathrm{C}$, the amount of a solute $(\mathrm{mol} . \mathrm{wt}=100)$ to be added to $100 \mathrm{~g}$ of water $\left(K_{b}=0.5\right)$ is