Ethanol, C₂H₅OH, has a normal boiling point of 78.4 °C. At this temperature its molar enthalpy of vaporization is 38.6 kJ mol⁻¹.
(a) Calculate the quantity of heat, in kJ, that must be absorbed to convert 125 g of liquid ethanol at 78.4 °C completely to vapor at the same temperature.
(b) Determine the amount of heat, in J g⁻¹, that would be released if one gram of ethanol vapor at 78.4 °C were condensed to liquid at the same temperature. Express your answer to three significant figures and include the appropriate sign.