Calculate the mass of a non-volatile solute of molar mass `40gmol^(-1)` which when disolved in 114g octane to reduce it vapour presure to 80%.

Calculate the mass of a non-volatile solute of molar mass 40 which should be dissolved in 114g octane to reduce its vapour pressure to 60%

Calculate the mass of compound ( molar mass = 256 g mol^(-1) ) to be dissolved in 75 g of benzene to lower its freezing point by 0.48 K (Kf= 5.12 K kg mol^(-1)) .

100 g of liquid A (molar mass 140 g mol^-1) was dissolved in 1000g of liquid B (molar mass 180 g mol^-1) . The vapour pressure of pure liquid B was found to be 500 torr: Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 Torr.

Urea [NH_2)_2CO] forms an ideal solution in water. Calculate the vapour pressure of an aqueous solution containing 5% by mass of urea at 298K. At 298K, vapour pressure of water is 23.75 mm Hg.

A 0.1539 molal aqueous solution of canesugar (molar mass = 342g mol^-1) has a freezing point 271K. While the freezing point of pure water is 273.15k. What will be the freezing point of an aqueous solution, containing 5g of glucose (Mol mass = 180g mol^-1) per 100g of solution?

A solution containing 30g of non-volatile solute exactly in 90g of water has a vapour pressure of 2.8 kPa at 298 K. Further, 18 g of water is then added to the solution and the new vapour pressure becomes 2.9 kPa at 298 K. Calculate: molar mass of the solute

Calculate the concentration of nitric acid in molarity in a sample which has a density, 1.41g/ml and contain 49% by mass of nitric acid

A solution containing 15g urea (molar mass = 60g/mol) per litre of solution in water is isotonic with the solution of glucose (molar masss 180g//mol ) in water calculate the mass of glucose present in one litre of its solution,.

An aqueous solution of 2 percent non-volatile solute exerts a pressure of 1.004 bar at the normal boiling point of the solvent. What is the molecular mass of the solute?

Ethylene glycol (molar mass = 62gmol^-1) is a common automobile antifreeze. Calculate the freezing point of a solution containing 12.4g of this substance in 100g of water. Would it be advisable to keep this susbtance in the car radiators during summer? Given K_f for water = 1.86 K kg//mol K_b for water = 0.612 K kg//mol