Question

The molar heat of fusion of chloroform (CHCl3) is 8.80 kJ/mol at its normal melting point of -63.6 *C. The molar heat of vaporization of chloroform is 31.4 kJ/mol at its normal boiling point of 61.7 *C. Calculate the heat required to melt 11.5g of chloroform at its normal melting point. Calculate the heat required to vaporize 11.5g of chloroform at its normal boiling point?

Answer 1

please help

Answer 2

first, you'll need to convert 11.5g of chloroform to moles.

the molar mass of CHCl3 is 119.38g/mol, so simply divide (11.5g) / (119.38 g/mol)

now, to get the heat required to melt chloroform at its melting point
---> (# of moles) * (molar heat of fusion)
(in chemistry, fusion is the same thing as melting)

to get the heat required to vaporize chloroform at its vaporization point:
---> (# of moles) * (molar heat of vaporization)