One liter aqueous solutions contains `2 xx 10^(-2)` kg glucose at `25^@C` . Calculate the osmotic pressure of the solution.

100 mL of an aqueous solution of protein contais 6.3 g of protein. Calculate the molar mass of protein if osmatic pressure of the solution at 27^@C is 2.57 xx 10^(-3) bar.

The partial pressure of ethane over a solution containing 6.50 xx10^(-3) g of ethane is 1 bar. If the solution contains 5.00 xx10^(-2) g of ethane, then what shall be the partial pressure of the gas?

200" cm"^(2) of an aqueous solution of a protein contains 1.26 g of the protein. The oxmotic pressure of such a solution at 300 K is found to be 2.57xx10^(-3) bar. Calculate the molar mass of the protein.

300 mL of an aqueous solution of a protein contains 2.52 g of the protein. If osmotic pressure of such a solution at 300 K is 5.04xx10^(-3) bar, the molar mass of the protein in g mol^(-1) is

Solution S_1 contains 3g of urea per litre and solution S_2 contains 9g glucose per litre. At 298 K, the osmotic pressure of

18 g glucose and 6 g urea are dissolved in 1L of solution at 27^@C , the osmotic pressure in atm of the solution will be