Homework Help: Chemistry

Posted by Anonymous on Thursday, February 11, 2010 at 9:24pm.

How much heat is required to convert 32.5 grams of ethanol at 28 C to the vapor phase at 78 C?

Ethanol (C2H5OH) boils at 75 C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g-K.

Chemistry - drwls, Thursday, February 11, 2010 at 9:45pm
First convert 32.5 g to moles. The molecular weight of C2H5OH is 24 + 16 + 6 = 46
You have 32.5/46 = 0.707 moles of ethanol.

The heat required (in kJ) is
0.707*38.56 + 32.5*50*2.3*10^-3
Chemistry - Anonymous, Thursday, February 11, 2010 at 11:47pm
31

Answer this Question

Related Questions

Chemistry - When 25.0 g of ethanol vapor condenses, 23.6 kJ of heat is released...
Chemistry - How much energy (in kilojoules) is released when 26.5 of ethanol ...
Chemistry - Search: How much energy (in Kj) is relased when 25.0g of ethanol ...
chemistry - the specific heat of ethanol is o.58 cal/g c how much energy is ...
Physics - How much heat is required to melt 50 grams of ice heat it to its ...
Chemistry - Ethanol (C2H5OH) boils at a temperature of 78.3oC. What amount of ...
chemistry - Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is 5....
Chemistry - The molar heat of vaporization of ethanol is 43.5 kJ/mo. Calculate ...
Chemistry - How much energy (in kilojoules) is released when 26.5g of ethanol ...
Chemistry - Ethanol burns to produce 1300.0 kJ/mol and has a heat capacity of 65...

For Further Reading

First Name:
School Subject:
Answer: