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?

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

Which of the following aqueous solutions containing 10g of solute in each case, has highest melting point?

A flask contains 3g H_(2) and 24g O_(2). The partial pressure of hydrogen in the mixture 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

A container of just 10cc has 2.69 xx 10^20 gas molecules at 0^@C . What is the pressure exerted?

At 50^@C the vapour pressure of H_2O is 92mm Hg. The vapour pressure of a solution containing 18.1g of non volatile solute in 100ml H_2O at the same temperature is 87mm Hg. Find the molecular weight of the solute.

In a ten litre vessel, the total pressure of a gaseous mixture containing H_(2), N_(2) and CO_(2) is 9.8atm. The partial pressures of H_(2) and N_(2) are 3.7 and 4.2 atm respectively. Then the partial pressure of CO_(2) is

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

For the equilibrium 2SO_3(g) leftrightarrow 2SO_2(g)+O_2(g) the partial pressure SO_3,SO_2 and O_2 gases , at 650 K are respectively 0.3 bar ,0.6 bar and 0.4 bar. IF the moles of both the oxides of sulphur are so adjusted as equal, what will be the partial pressure of O_2 .

At 300K, the osmotic pressue of 300mL of a protein aqueous solution is 8.3 xx 10^(-5) bar. The molar mass of protein is 10^4 "gmol^(-1) . What is the weight (in g) of the protein present in this solution ? (R=0.083 L bar "mol"^(-1) K^(-1) )