Henry's law constant for CO2 in water at 298 K is $1.67 imes 10^8$ Pa. Calculate the mass of CO2 that can be dissolved in 500 mL of water at 298 K and a CO2 partial pressure of 2.5 atm.

Binary liquid solutions which exhibit negative deviations from Raoult’s law boil at temperature ….than the expected value :

When 25 g of a non-volatile solute is dissolved in 100 g of water, the vapour pressure is lowered by $2.25 imes {10^{ - 1}}\;{\rm{mm}}{\rm{.}}$ If the vapour pressure of water at $20^\circ C$ is 17.5 mm, what is the molecular weight of the solute?

The vapour pressure of benzene at $80^\circ C$ is lowered by 10 mm by dissolving 2g of a non-volatile substance in 78 g of benzene. The vapour pressure of pure benzene at $80^\circ C$ is 750 mm. The molecular weight of the substance will be :

On mixing, heptane and octane form an ideal solution. At 373 K, the vapour pressures of the two liquid components (heptanes and octane) are 105 kPa and 45kPa respectively. Vapour pressure of the solution obtained by mixing 25 g of heptanes and 35 g of octane will be (molar mass of heptanes $= 100\;g\;mo{l^{ - 1}}\;$ and of octane $= 114\;g\;mo{l^{ - 1}}\;$

Two liquids X and Y form an ideal solution. The mixture has a vapour pressure of 400 mm at 300 K when mixed in the molar ratio of 1:1 and a vapour pressure of 350 mm when mixed in the molar ratio of 1:2 at the same temperature. The vapour pressures of the two pure liquids X and Y respectively are

The mixture that forms maximum boiling azeotrope is:

Positive deviation is observed in case of

An aqueous solution of methanol in water has vapour pressure

If liquids A and B form an ideal solution, the

When two liquids A and B are mixed then their boiling points becomes greater than both of them. What is the nature of this solution?