Ethanol (C₂H₅OH)burns according to the equation C₂H₅OH(l)+ 3O₂(g) $\rarr$ 2CO₂(g)+ 3H₂O(l), $\Delta$H°_rxn = -1367 kJ/mol. How much heat is released when 35.0 g of ethanol is burned? A)9.61 × 10^-4 kJ B)1,040 kJ C)1,367 kJ D)1,797 kJ E)4.78 × 10⁴ kJ

Question

Quizplus · Accepted Answer

The molar mass of ethanol is 46.08 g/mol. 35.0 g of ethanol is 35.0 g / 46.08 g/mol = 0.759 mol. The heat released is 0.759 mol × (-1367 kJ/mol) = -1038.9 kJ, which rounds to 1,040 kJ.

Ethanol (C2H5OH)burns According to the Equation C2H5OH(l)+ 3O2(g) →\rarr→ 2CO2(g)+ 3H2O(l) Δ\DeltaΔ

Ethanol (C₂H₅OH)burns According to the Equation C₂H₅OH(l)+ 3O₂(g) $\rarr$ 2CO₂(g)+ 3H₂O(l) $\Delta$