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04/10/2021 3:55 pm
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For complete combustion of ethanol,
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l),
the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol-1 at 25ºC. Assuming ideality the enthalpy of combustion, ΔcH, for the reaction will be: (R = 8.314 kJ mol-1)
(a) -1366.95 kJ mol-1
(b) -1361.95 kJ mol-1
(c) -1460.95 kJ mol-1
(d) -1350.50 kJ mol-1
1 Answer
1
04/10/2021 4:00 pm
Correct answer: (a) -1366.95 kJ mol-1
Explanation:
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l)
Bomb calorimeter gives DU of the reaction
Given, ΔU = –1364.47 kJ mol-1
Δng = -1
ΔH = ΔU + ΔngRT
= -1364.47 - \(\frac{1 \times 8.314 \times 298}{1000}\)
= -1366.95 kJ mol-1