Question

C2H5OH( l) + 3O2( g) → 2CO2( g) + 3H2O( l); Δ H = –1.37 × 103 kJ Consider the following propositions: I. The reaction is endothermic II. The reaction is exothermic. III. The enthalpy term would be different if the water formed was gaseous. Which of these propositions is (are) true?

Answer 1

II. The reaction is exothermic.

III. The enthalpy term would be different if the water formed was gaseous.

Step-by-step explanation:

For the reaction:

C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l)

The ΔH is -1.37×10³ kJ. As the change in enthalpy is <0, II. The reaction is exothermic.

The ΔH formation of a compound is different if the chemical is in liquid or gaseous phase. For that reason: III. The enthalpy term would be different if the water formed was gaseous.

I hope it helps!