`2000 cm^3` of an aqueous solution of a protein contains 1.26 g of the protein. The osmotic pressure of such a solution at 300K is found to be 2.57 …`10^(-3)` bar. Calculate the molar mass of the protein.

100 mg of a protein is dissolved in just enough water to make 10.0 mL of solution. If this solution has an osmotic pressure of 13.3mm Hg at 25^@C , what is the molar mass of the protein? (R = 0.0821L atm mol^-1 K^-1 and 760mm Hg = 1atm)

Calculate the molarity of a solution containing 1g of NaOH in 250 mL of water.

Benzene and toluene form ideal solution over the entire range of composition. The vapour pressure of pure benzene and toulene at 300 K are 50.71 mm Hg and 32.06 mm Hg respectively. Calculate the mole fraction of benzene in vapour phase if 80 g of benzene is mixed with 100 g of toluene.

Rate constant K for a first order reaction has been found to be 2.54xx10^(-3)sec^(-1) Calculate its 3//4 the life (log 4=0.6020)

At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration?

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?

Calculate molarity of a solution containing 11.7g NaCl in 2.0L solution.

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.

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