Using ?Hfus= [RT*2/?T] xB
where
R = 8.31451 J K-1 mol-1 gas constant
T* = 273.15 freezing point of the pure solvent in Kelvin
?Hfus = the enthalpy of fusion of the solvent
XB = 0.009174 the mole fraction of the solute
unsure of what ?T is we were giving the equation
?T = Kf mB
?T = the freezing point depression
Kf = the cryoscopic constant of the solvent
mB= the molarity of the solution, or the number of moles of solute per kilogram of solvent.
do i use the answer obtained from this to find ?Hfus?
the solvent was cycloheane and the solute was napthalene
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Topic: Help calculating the enthalpy of fusion (Read 9134 times)