A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 24.1 g of the compound in water to form 0.250 L solution. The solution so formed has an osmotic pressure of 1.99 atm at 25°C. Assuming that the organic compound is a nonelectrolyte, what is its molar mass?
I set up the problem using the osmosis equation as:
1.99atm = (.0821)(298.15)(M)
The Molarity is .0813mol/1L
I found the number of moles to be .0203 by multiplying (.0813mol)(.25L)
I don't know what to do next