Problem: Three common hydrocarbons that contain four carbons are listed here, along with their standard enthalpies of formation:HydrocarbonFormulaHf(kJ/mol)1,3-ButadieneC4 H6 (g)111.91-ButeneC4 H8 (g)1.2n-ButaneC4 H10 (g)-124.7For 1,3-Butadien calculate the molar enthalpy of combustion to CO2 (g) and H2 O(l).

FREE Expert Solution

We are asked to calculate the molar enthalpy of combustion to CO2 (g) and H2O(l) for 1,3-Butadiene.


ΔH°rxn=ΔH°f, prod-ΔH°f, react


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) 


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Problem Details
Three common hydrocarbons that contain four carbons are listed here, along with their standard enthalpies of formation:


HydrocarbonFormulaHf(kJ/mol)
1,3-ButadieneC4 H6 (g)111.9
1-ButeneC4 H8 (g)1.2
n-ButaneC4 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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