Ethane combusts completely, in accordance with this chemical pathway: 2C↓2H↓6(g) + 7O↓2(g) > 4CO↓2(g) + 6H↓2O(g), ΔH = ?
The enthalpies of the following elementary steps are known:
2C(s) + 3H↓2(g) > C2H↓6(g), ΔH = -84.7kJ/mol
C(s) + O↓2(g) > CO↓2(g), ΔH = -394kJ/mol
H2(g) + (1/2)O2(g) > H2O(g), ΔH = -242kJ/mol
Use the known enthalpies to determine the overall enthalpy of the process described in the balanced combustion equation above.