Calculate the total amount of energy (in kJ) necessary to raise the temperature of 2.00 L of ethanol (density = 0.7849 g/cm3) from 18 0C to its boiling point (78.3 0C) and then to fully vaporize the liquid. Assume that it is a closed system where no heat exchange with the surroundings take place. Given: Cethanol = 2.44 J/g·K; heat of vaporization of ethanol at 78.3 0C = 38.56 kJ/mol.

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