Consider the reaction: C2H5OH(ℓ) + 3O2(g) → 2CO2(g) + 3H2O(ℓ); ∆H = –1.37 x 103 kJ Consider the following statements: 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 statement(s) is (are) true?

Two statements are true:

II. The reaction is exothermic. III. The enthalpy term would be different if the water formed was gaseous.

Explanation:

C₂H₅OH(ℓ) + 3O₂(g) → 2CO₂(g) + 3H₂O(ℓ); ∆H = –1.37 × 10³ kJ

1. ∆H = –1.37 × 10³ kJ it telling that the enthalpy of the reaction is negative.

That means that reaction releases heat, which, by definition, means that the reaction is exothermic.

Then statement I is false and statement II is true.

2. The enthalpy of a reaction is equal to the enthalpy of the products less the enthalpy of the reactants:

       

The enthalpy of each substance depends on its state, thus the enthalpy term for water will be different if it is formed as a gas than if it is formed a liquid.

Hence, the enthalpy of the reaction will be different in case the water formed was gaseous, and the third statement is also true.

Forgot the question hahaha

Elias is almost correct. he just got it backwards.the correct answer is that it demonstrates elastic potential energy transforming into kinetic energy.