a)
Hcombustion = Qcombustion / moles
Q = 99.472 kJ
n = mass/MW = 3.365/46 = 0.0731521 mol of ethanol
HRcomb = (99.472/0.0731521) = 1359.79 kJ/mol
b)
Hf for ehtanol given:
C2H5OH(l) + O2 (g)= CO2(g) + H2O(g)
balance:
C2H5OH(l) + 3O2 (g)= 2CO2(g) + 3H2O(g)
HRxn = Hproducts - Hreactants
1359.79 = (2*-393.5 + 3*-241.818) - (C2H5OH + 3*0)
C2H5OH = 1359.79- (2*-393.5 + 3*-241.818)
C2H5OH = 2,872.24 kJ/mol
4.20 If 3.365 g of ethanol C_2H_5OH(l) is burned completely in a bomb calorimeter at 298.15...
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