How much heat is required to convert 35.0 g of ethanol at -168 ∘C to the vapor phase at 78 ∘C?
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Expert's answer
2016-12-06T14:51:11-0500
The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g−K. q = m x C xΔT + m (ΔH/M) q = 35.0g x 2.3J/goC x (78 + 168)oC + 35.0g x 837 J / g q = 19803 J + 29295 J = 49.09 kJ Answer 49.09 kJ
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