10 g of solute A and 20 g of solute B both are dissolved in 500 mL of water. The solution has the same osmotic pressure as 6.67 g of A and 30 g of B are dissolved in the same volume of water at the same temperature. What is the ratio of molar masses of A and B ?

. 3.7 g of a gas at 25^@C occupied the same volume as 0.184 g of hydrogen at 17^@C and at the same pressure. What is the molar mass of the gas ?

Find the osmotic pressure of a solution at 27^@C when 10 gm Glucose and 6 gm urea is dissolved in 500 ml water.

2.9 g of a gas at 95^(@)C occupied the samme volume as 0.184 g of dhydrogen at 17^(@)C , at the same pressure, what is the molar mass of the gas?

Calculate the volume of 3.6g of water vapour at 273K temperature and 1 atm pressure.

The mass of glucose that should be dissolved in 100 g of water in order to produce same lowering of vapour pressure as is produced by dissolving 1 g of urea in 50 g of water is

20 g of NaOH is present in 250 mL of H_(2) O . Calculate the active mass of the solution .

When 2 g of a gas 'M' is introduced into an empty flask at 30^(@)C , its pressure becomes 1 atm. Now, if 3g of another gas 'N' is introduced in the same flask at the same temperature, the total pressure becomes 1.5 atm. Find the ratio of the molar masses of the two gases.

A solution containing 6 gm of a solute dissolved in 250 ml of water gave an osmotic pressure of 4.5 atmosphere at 27^(@)C . Calculate the boiling point of the solution. The molal elevation constant for water is 0.52

58.4 g of NaCI and 180 g of glucose were separately dissolved in 1000 mL of water. Identify the correct statement regarding the elevation of boiling point (b.p.) of the resulting solutions.

How many g of KCl would have to be dissolved in 60 g H_2O to give 20% by weight of solution ?