When 8.97 g of a non-electrolyte is dissolved in water to make 620 mL of solution, an osmotic pressure of 1.80 torr, measured at 29 °C.?

van't Hoff factor, i = 1  (for non-electrolyte)
Molarity, c = (8.97/y mol) / (620/1000 L) = 14.47/y M
Gas constant, R = 0.08206 L atm / (mol K)
Temperature, T = (273 + 29) K = 302 K
Osmotic pressure, Π = 1.80/760 atm

Π = i c R T
1.80/760 = 1 × (14.468/y) × 0.08206 × 302
y = 14.47 × 0.08206 × 302 × (760/1.80)
y = 1.51 × 10⁵

Molar mass of the electrolyte = 1.51 × 10⁵ g/mol

https://en.wikipedia.org/wiki/Osmotic_pressure