2C2H6(g) + 5O2(g) → 4CO2(g) + 2H2O(g) ΔH = -2511 kJ

The enthalpy change (ΔH) for this reaction is -2511 kJ, which indicates that the reaction is exothermic. This means that heat is released during the course of the reaction.

Exothermic reactions are typically favored at lower temperatures because the release of heat helps to drive the reaction forward. As the temperature increases, the equilibrium shifts towards the reactants, and the reaction becomes less efficient at converting reactants to products.