I just need to make sure I did this correctly...
If we dissolve 84.9mg of an unknown molecular material in 100.0mL of water, the resulting solution has an osmotic pressure of 188 torr at 27.0 degrees Celsius. What is the molar mass of the unknown material?
84.9mg/100mL = 0.849g/L
188 torr * (1 atm/760 torr) = 0.247 atm
27 + 273 = 300K
Then, I just plugged everything in.
0.247atm = (0.849g/molar mass)(0.0821)(300K)
And rearranged to solve for molar mass and ended up with 84.66g/mol.
Is this correct?