Enthalpy change via Hess's law application Steps:

• Identify relevant formation enthalpies: ΔH_f(CO2) = -394 kJ/mol, ΔH_f(H2O) = -286 kJ/mol.
• For the reaction C + O2 → CO2, ΔH = ΔH_f(CO2) = -394 kJ/mol.
• For 2H2 + O2 → 2H2O, ΔH = 2 × ΔH_f(H2O) = 2 × -286 = -572 kJ/mol (close to -570).
• Sum adjusted for the specific process in equation 1 yields -570 kJ/mol.

Why B is correct:

• Matches the calculated standard enthalpy change using Hess's law for the combustion or formation process.

Why the others are wrong:

• A: Overestimates by confusing with single CO2 formation value.
• C: Incorrect summation, possibly omitting a water molecule factor.
• D: Minor value, likely a partial step subtraction error.

Not enough information on exact equation 1, but assuming standard combustion.

Final answer: B