# Problem: Three common hydrocarbons that contain four carbons are listed here, along with their standard enthalpies of formation:HydrocarbonFormulaΔH˚f(kJ/mol)1,3-ButadieneC4H6(g)111.91-ButeneC4H8(g)1.2n-ButaneC4H10(g)–124.7For 1,3-Butadiene, calculate the fuel value in kJ/g.

###### FREE Expert Solution

We are asked to calculate the fuel value in kJ/g 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)

ΔH°rxn = -2411.3 kJ

Molar mass C4H6(g) = 54.10 g/mol

88% (443 ratings) ###### Problem Details
Three common hydrocarbons that contain four carbons are listed here, along with their standard enthalpies of formation:
 Hydrocarbon Formula ΔH˚f(kJ/mol) 1,3-Butadiene C4H6(g) 111.9 1-Butene C4H8(g) 1.2 n-Butane C4H10(g) –124.7

For 1,3-Butadiene, calculate the fuel value in kJ/g.

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