C₂H₅OH(l) + 3O₂(g) $\rightarrow$2CO₂(g) + 3H₂O(l), $\Delta$H = -1.37 * 10³ kJ For the combustion of ethyl alcohol as described in the above equation, which of the following statements is(are) true? I. The reaction is exothermic. II. The enthalpy change would be different if gaseous water were produced. III. The reaction is not an oxidation-reduction one. IV. The products of the reaction occupy a larger volume than the reactants.

Question

Quizplus · Accepted Answer

The reaction is exothermic as indicated by the negative enthalpy change. The enthalpy change would differ if gaseous water were produced due to the difference in phase enthalpy.

C2H5OH(l) + 3O2(g) →\rightarrow→ 2CO2(g) + 3H2O(l) Δ\DeltaΔ H = -137 * 103 KJ for the Combustion of Ethyl Alcohol

C₂H₅OH(l) + 3O₂(g) $\rightarrow$ 2CO₂(g) + 3H₂O(l) $\Delta$ H = -137 * 10³ KJ for the Combustion of Ethyl Alcohol