Answer:
30.5 g of estrogen
Explanation:
Lowering vapor pressure formula → P° - P' = P° . Xm
P° → Vapor pressure of pure solvent → 54.68 mmHg
P' → Vapor pressure of solution → 53.46 mmHg
54.68 mmHg - 53.46 mmHg = 54.68 mmHg . Xm
0.0223 = Xm → This is the mole fraction for solute
Moles of solute / Total moles
Total moles = Moles of solute + Moles of solvent
Let's determine the moles of solvent → 228 g / 46.07 g/mol = 4.95 moles
Let's determine the moles of solute
Moles of solute / Moles of solute + 4.95 = 0.0223
Moles of solute = 0.0223 . Moles of solute + 0.110
0.9777 moles of solute = 0.110
Moles of solute = 0.110 / 0.9777 → 0.112
Now we can convert the moles to mass to finish the excersise:
0.112 mol . 272.4 g/mol = 30.5 g
