How much energy is released when 15.34 g of ethanol (C2H5OH) gas at 300 °C is converted to liquid ethanol at 2?
Boiling point,
78.5°C
Heat of vaporization,
879 J/g
Specific heat capacity, C2H5OH(g)
1.43 J/(g.°C)
Specific heat capacity, C2H5OH(l)
2.45 J/(g.°C)
Answer
30.6 kJ
23.1 kJ
18.9 kJ
20.4 kJ
15.4 kJ
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Verified answer
To go from a gas at 300 deg to a gas at 78.5 deg = 15.43 g x 1.43 J/gC x 221.5 = 4887.4 J
To go from a gas at 78.5 deg C to a liquid at 78.5 deg = 15.34 g x 879 J/g = 13483.9 J
To go from liquid at 78.5 deg to liquid at 2 deg deg = 15.34 g x 2.45 J/gC x 76.5 = 2875.1
Some how I get 21.2 kJ
Check my math and my steps, but this is essentially the approach to take.