Problem: Ethanol (C2H5OH) melts at -114°C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g•K and 2.3 J/g•K respectively. How much heat (kJ) is required to convert 24.0 g of ethanol at 21°C to the vapor phase at 78°C? Express your answer using two significant figures. 

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Ethanol (C2H5OH) melts at -114°C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g•K and 2.3 J/g•K respectively. 

How much heat (kJ) is required to convert 24.0 g of ethanol at 21°C to the vapor phase at 78°C? 

Express your answer using two significant figures. 



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Based on our data, we think this problem is relevant for Professor Casey's class at UNR.