Answer:
29.625 kJ.
Explanation:
Enthalpy of vaporization, ∆Hvap which is also known as the latent heat of vaporization, is the amount of energy required to be added to a liquid substance to change the phase of a quantity of that substance into a gas.
Molar mass of Isopropyl alcohol (C3H80) = (12*3) + (1*8) + 16
= 60 g/mol.
Number of moles = mass*molar mass
= 39.5*60
= 0.658 moles.
Heat required = n * molar enthalpy of vapourisation.
∆Hvap = 45 kJ/mol.
= 0.658*45
= 29.625 kJ.
