Answer:
ΔH° = 676 kJ
Explanation:
The approximate enthalpy change of the combustion of methane can be obtained by subtracting the enthalpies of the reactants from the products. The combustion of methane is shown using the chemical equation below:
C[tex]H_{4}[/tex] + 2[tex]O_{2}[/tex] ⇔ 2[tex]H_{2}O[/tex] + C[tex]O_{2}[/tex]
Therefore, the approximate enthalpy change is:
ΔH° = 2*(Δ[tex]H_{H_{2}O }[/tex]) + Δ[tex]H_{CO_{2} }[/tex] - Δ[tex]H_{CH_{4} }[/tex] - 2*(Δ[tex]H_{O_{2} }[/tex]) = 2(928)+1472-1656-2(498) = 676 kJ
The approximate enthalpy change is 676 kJ.
We used only the magnitude of the enthalpies for the calculation.
