CH4(g) + 2O2(g) → 2H2O(l) + CO2(g) ∆H = 890KJ mo-1 ∆H in the reaction represented by the equation above is the enthalpy of

CH_4(g) + 2O_{2(g) → 2H2O(l) + CO2(g) ∆H = 890KJ mo-1 ∆H in the reaction represented by the equation above is the enthalpy of}

Answer Details

The ∆H in the given chemical equation refers to the enthalpy change or heat change of the reaction. It is the difference between the enthalpy of the products and the enthalpy of the reactants. In this equation, energy is released in the form of heat (exothermic reaction), and the value of ∆H is 890KJ mo-1. Since the reactants in the equation include CH4 and O2, which are the typical fuels used in combustion reactions, it can be concluded that the reaction is a combustion reaction. Therefore, the correct answer is "combustion".