We are asked to calculate the molar enthalpy of combustion to CO2 (g) and H2O(l) for 1,3-Butadiene.
Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol.
Also, note that ΔH˚f for elements in their standard state is 0.
Balanced reaction:
C4H6(g) + 11/2 O2(g)→ 4 CO2(g) + 3 H2O(g)
Hydrocarbon | Formula | Hf(kJ/mol) |
1,3-Butadiene | C4 H6 (g) | 111.9 |
1-Butene | C4 H8 (g) | 1.2 |
n-Butane | C4 H10 (g) | -124.7 |
For 1,3-Butadien calculate the molar enthalpy of combustion to CO2 (g) and H2 O(l).
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