Final answer:
The enthalpy change (ΔH) for the combustion of naphthalene (C₁₀H₈) is almost equal to its heat of combustion at constant volume, which is -5133 kJ/mol, aligning with Option A.
Step-by-step explanation:
The determination of the enthalpy change (ΔH) during a chemical reaction is a fundamental aspect in chemistry. When given the heat of combustion at constant volume (ΔE), which is the heat released when one mole of a substance is burned in excess oxygen under constant volume conditions, the enthalpy change can be calculated. The heat of combustion of naphthalene (C₁₀H₈) at constant volume was found to be -5133 kJ/mol. The relationship between ΔH and ΔE at constant volume is given by the expression ΔH = ΔE + ΔnRT, where Δn is the change in the number of moles of gas, R is the ideal gas constant, and T is the temperature in kelvins.
However, for solid combustion, the change in the number of moles of gas is typically negligible, and hence the value of ΔH is often very close to that of ΔE. Therefore, for this case, we can consider the enthalpy change to be approximately equal to the heat of combustion. The correct option representing the enthalpy change of naphthalene's combustion is -5133 kJ/mol (Option A).