Asolution is made by dissolving 5.65 g of an unknown molecular compound in 110.0 g of benzene froze at 4.39 oc. what is the molar mass of the solute if pure benzene has a freezing point of 5.45 oc and the kf value of benzene is 5.07 oc/m

238.91 g/mol is the molar mass of the solute.

Explanation:

Mass of solute = 5.65 g

Molar mas of solute = M

Mass of solvent = 110.0 g = 0.110 kg

where,

=Depression in freezing point

= freezing point constant of solvent= 5.07°C/m

1 =van't Hoff factor

m = molality

Freezing point constant of benzene ,T= 5.45°C/m

T = 5.45°C , =4.39 °C

i = 1

M = 238.91 g/mol

238.91 g/mol is the molar mass of the solute.

i just learnt this recently but i need to look through my notes again