An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 ml of solution. the solution has an osmotic pressure of 1.2 atm at 25 °c. what is the molar mass (g/mole) of the compound?

M=n (pie) / RT

n=osmotic pressure (1.2 atm)

M=molar of the solution

R=gas constant (0.0821)

T = temperature in kelvin 25+273

M=[1.2atm / (0.0821L atm/k mol x 298k) ]=0.049mol L

M = moles of the solute / litres of solution (250/1000)

0.049 = y/0.25

moles of solute is therefore = 0.01225mol

molar mass=33.29 g/0.01225mol=2.7 x10^3g/mol