Consider the reaction
C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) , ΔH = -1.37 × 10³ kJ
When a 15.7-g sample of ethyl alcohol (molar mass = 46.1 g/mol) is burned, how much energy is released as heat?

Question

Quizplus · Accepted Answer

The energy released is calculated by first determining the moles of C2H5OH in 15.7 g, which is 15.7 g / 46.1 g/mol = 0.341 mol. The reaction releases -1.37 × 10^3 kJ per mole of C2H5OH, so the energy released is 0.341 mol × -1.37 × 10^3 kJ/mol = -467 kJ.

Consider the Reaction C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), ΔH = -1.37

Consider the Reaction C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l), ΔH = -1.37