Final answer:
To calculate the enthalpy change (ΔH) for the reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g), bond enthalpies for the bonds broken and formed would be needed, summing the energy required to break the reactant bonds and subtracting the energy released by forming product bonds.
Step-by-step explanation:
To calculate the enthalpy change (ΔH) for the reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g), we need to use the bond enthalpies for the bonds broken and formed during the reaction. Unfortunately, the given bond enthalpies are not directly provided in the question. However, the general approach to solve this would involve summing the bond enthalpies of all bonds broken in the reactants and subtracting the bond enthalpies of all bonds formed in the products.
The energy required to break bonds is always positive, and the energy released when bonds form is negative. Therefore, to estimate ΔH for the reaction, one would follow this equation: ΔH = Energy to break bonds - Energy to form new bonds. For a complete solution, we would need specific bond enthalpies for every bond in the reactants and products.