[laxplayer]

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
                             

[ARGOS++]

Dear Laxplyer;

If you got that the mass will be 0.0203 Moles, then how many Grams are that?
And I’m sure: Soon you will know what the MW of your organic compound is.

Good Luck!
                    ARGOS⁺⁺

[laxplayer]

Oh, 24.1g/.0203mol=1187.2

silly me :]

[ARGOS++]

Dear Laxplyer;

I see:  - I’m right!

Good Luck!
                    ARGOS⁺⁺