Use the References to access important values if seeded for

Use the References to access important values if seeded for this question In a laboratory experiment, a student found that a 186-mL, aqueous solution containing 2.329 g of a compound had an osmotic found to be nonvolatile and a nonelectrolyte. What is the molar mass of this compound? pressure of 12.5 mm He at 298 K. The compound was afso g mol Submin Answer

Solution

osmatic pressure = M * R * T

where, M = molarity

R = Gas constant

T = temperature

osmatic pressure = 12.5 mmHg = 0.0164 atm

0.0164 = M * 298

M = 5.50*10^-5 M

molarity = number of moles of solute / volume of solution in L

5.50*10^-5 M = number of moles of solute / 0.186 L

number of moles of solute = 5.50*10^-5 M * 0.186 = 1.02*10^-5 mol

number of moles of solute = mass / molar mass

1.02*10^-5 mol = 2.329 g / molar mass

molar mass = 2.329 g / 1.02*10^-5 mol = 2.28*10^-5 g/mol

Therefore, molar mass =  2.28*10^-5 g/mol