Answer:
201.8 g/mol is the molar mass for the compound
Step-by-step explanation:
To solve this, we apply the formula for freezing point depression:
Freezing point for solution = - (Kf . m - Freezing point por pure solvent)
Freezing point for solution = - Kf . m + Freezing point por pure solvent
Freezing point for pure solvent = 0°C, therefore - 0.820°C = - Kf . m
Kf = 1.86 °C/m ; m = molality (mol/kg), moles of solute in 1kg of solvent
It is more common to say 1.86 °C/m instead of K/m
0.820°C / 1.86 m°C = m → m = 0.441 molal (These moles are in 1kg of solvent, but our mass is 40 g, 1kg = 1000g)
We determine the moles of solute → Molal . mass of solvent
0.441 mol/1000g . 40 g = 0.0176 moles
Molar mass → mass of compound (g) in 1 mol → 3.56 g / 0.0176 moles = 201.8 g/mol