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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FREE Expert Solution
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Problem Details

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?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems .

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Our tutors rated the difficulty of Ethanol (C2H5OH) melts at -114°C and boils at 78°C. The enth... as high difficulty.

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Our expert Chemistry tutor, Dasha took 10 minutes to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Davis' class at UCF.