Consider ethanol (C2H5OH, or C2H6O) burning with air. The lower heating value (LHV) of ethanol is given as 26,700 kJ/kg. Compute the higher heating value (HHV) of ethanol in kJ/kg from the given LHV value and the enthalpy of vaporization of water (44,010 kJ/kmol).
Answer
29564 kJ/kg
Explanation
Balanced equation for combustion of ethanol is
C2H5OH(l) + 3O2(g) -----> 2CO2(g) + 3H2O(g)
nH2O,out/ nfuel ,in = 3/1 =3
HHV = LHV + Hv( nH2O,in/ nfuel, in )
Hv = Heat of vaporization of water, 44..010kJ/mol =
LHV = 1230.3kJ/mol
HHV = 1230.3 kJ/mol + (44.010kJ/mol × 3 )
HHV = 1230.3 kJ /mol + 132.03kJ/mol
HHV = 1362.3 kJ/mol
HHV = 29564 kJ/kg
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