Answer
see solution
Work Step by Step
Given mass of solute, $C_6H_{12}O_6$= 55.8g
mass of 1 mole of solute= 180g
moles of solute = ((1/180)x55.8)= 0.3 moles
Mass of solvent = 0.45 kg
Molality= moles of solute/mass of solvent
= 0.3moles/0.455 kg = 0.65 mol/kg
dTb= (molality x Hvap )
Heat of vaporization= 0.512 C kg/mol
Now dTb= 0.65 m x 0.512 Ckg/mol= 1.26 C
Freezing point= 0-1.26C= -1.26C
dTb= (molality x Hfusion )
Heat of fusion= 1.86 C kg/mol
Now, dTb = 0.65 m x 1.86 Ckg/mol= 0.35 C
Boiling point = 100+0.35 =100.35 C
