It is true that the complete combustion of a hydrocarbon can do more work than incomplete combustion. Compare the work ΔG done by the combustion of one mole of ethane undeer these conditions.
Incomplete combustion: 2 C2H6 (g) + 5 O2 (g) → 4 CO(g) + 6 H2O (g)
Complete combustion: 2 C2H6 (g) + 7 O2 (g) → 4 CO(g) + 6 H2O (g)
can someone please help me solve this problem? and show how it is done.
thank you
2007-12-07 08:19:33 · 1 answers · asked by abc 1 in Science & Mathematics ➔ Chemistry
In your text, you should have a table of the free energies of formation of a bunch of compounds, including all those in this table. You also know that the free energy of formation of an element (like 02) is 0.
You can calculate the free energy change (DG) for any reaction by adding up the free energies of formation of each of the products and subtracting the free energy of formation of the reactants. For each substance, be sure to multiply the value by the coefficient in the balanced equation.
Hopefully that'll get you there...
2007-12-07 08:33:28 · answer #1 · answered by hcbiochem 7 · 0⤊ 0⤋