Henry’s law constant for the solution of methane in benzene at 298 K is 4.27 × 10⁵ mm Hg. The mole fraction of methane in benzene at 298 K under 760 mm Hg will be:

1. 1.85 × 10^–5

2. 192 × 10^–4

3. 178 × 10^–5

4. 18.7 × 10^–5

The solubility of gases in liquids generally decreases as temperature increases.
The primary reason for this behavior is:

Which law is applied when deep-sea divers use a breathing mixture of oxygen and less soluble helium to minimise the painful effects caused by the increased dissolution of gases in blood at high pressure?

Which graph represents the positive deviation of vapor pressure?

1.		2.
3.		4.	None of the above

The following solutions were prepared by dissolving 10 g of glucose (C₆H₁₂O₆) in 250 ml of water (P₁), 10 g of urea (CH₄N₂O) in 250 ml of water (P₂) and 10 g of sucrose (C₁₂H₂₂O₁₁) in 250 ml of water (P₃). The decreasing order of osmotic pressures of these solutions is:

The correct option for the value of vapour pressure of a solution at 45 $°$C with benzene to octane in a molar ratio 3:2 is:

[At 45 $°$C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume Ideal gas]

At room temperature, a dilute solution of urea is prepared by dissolving 0.60 g of urea in 360 g of water. If the vapour pressure of pure water at this temperature is 35 mm Hg, then calculate the lowering of vapour pressure:
(Given: Molar mass of urea = 60 g mol^–1)

The mole fraction of glucose (C₆H₁₂O₆) in an aqueous binary solution is 0.1. The mass percentage of water in it to the nearest integer is:

The type of inter-molecular interactions present in: