Calculate the change in enthalpy (ΔH) for the combustion of 1 mole of methane (CH4) to produce carbon dioxide (CO2) and water (H2O), given standard enthalpy changes of formation.
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To calculate the change in enthalpy (ΔH) for the combustion of 1 mole of methane (CH4) to produce carbon dioxide (CO2) and water (H2O), we need to use the standard enthalpy changes of formation.
The balanced chemical equation for the combustion of methane is:
CH4 + 2O2 -> CO2 + 2H2O
The standard enthalpy change of formation (ΔHf) for methane is -74.8 kJ/mol.
The standard enthalpy change of formation (ΔHf) for carbon dioxide is -393.5 kJ/mol.
The standard enthalpy change of formation (ΔHf) for water is -285.8 kJ/mol.
ΔH = ΣΔHf(products) - ΣΔHf(reactants)
ΔH = [ΔHf(CO2) + 2ΔHf(H2O)] - [ΔHf(CH4) + 2ΔHf(O2)]
ΔH = [-393.5 kJ/mol + 2(-285.8 kJ/mol)] - [-74.8 kJ/mol + 2(0 kJ/mol)]
ΔH = -787.1 kJ/mol - (-74.8 kJ/mol)
ΔH = -712.3 kJ/mol
Therefore, the change in enthalpy (ΔH) for the combustion of 1 mole of methane to produce carbon dioxide and water is -712.3 kJ/mol.
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