0.125 of an unknown nonelectrolyte compound dissolved in 100 ml?

For nonelectrolyte, van't Hoff index, i = 1
Osmotic pressure, Π = 30.1/760 atm
Gas constant, R = 0.08206 L atm / mol K
Temperature, T = (273 + 20) K = 293 K

Π = iMRT, then M = Π/(iRT)

Molarity, M = (30.1/760) / (1 × 0,08206 × 293) mol/L = 0.001647 mol/L

Number of moles of the compound = (0.001647 mol/L) × (100/1000 L) = 0.0001647 mol
Molar mass of the compound = (0.125 g) / (0.0001647 mol) = 759 g/mol

(30.1 mmHg) / (62.36367 L mmHg/K mol) / (20 + 273) K x (0.100 L) =
0.000164728 mol

Supposing the missing units on "0.125" to be "grams":
(0.125 g) / (0.000164728 mol) = 758.826 g/mol = 759 g/mol