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?

II. The reaction is exothermic.

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

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!

where's the diagram?

i'm assuming that it's c.) red bank..