Consider the reaction: C₂H₅OH(l)+ 3O₂(g)$\to$ 2CO₂(g)+ 3H₂O(l);$\Delta$H = -1.37 $\times$ 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?

Question

Quizplus · Accepted Answer

The reaction is exothermic because the enthalpy change ($\Delta H$) is negative (-1.37 x 10^3 kJ), indicating that heat is released. The enthalpy term would indeed be different if the water formed was gaseous because the physical state of products and reactants affects the enthalpy of the reaction.

Consider the Reaction: C2H5OH(l)+ 3O2(g) →\to→ 2CO2(g)+ 3H2O(l); Δ\DeltaΔ H = -137 ×\times×

Consider the Reaction: C₂H₅OH(l)+ 3O₂(g) $\to$ 2CO₂(g)+ 3H₂O(l); $\Delta$ H = -137 $\times$