Question

Consider the following thermochemical equation for the combustionof acetone, C3H6O, the main ingredient innail polish remover.C3H6O(l) + 4O2 (g) --->3CO2 (g) + 3H2O (g), ΔHoof the reaction = -1790 kcalIf a bottle of nail polish remover contains 177 mL of acetone,how much heat would be released by its complete combustion? Thedensity of acetone is 0.788 g/mL.

Answer 1

Answer:

-4.30 × 10³ kcal

Explanation:

Let's consider the following thermochemical equation for the combustion of acetone.

C₃H₆O(l) + 4 O₂ (g) → 3 CO₂(g) + 3 H₂O(g) ΔH°of the reaction = -1790 kcal

When 1 mole of C₃H₆O burns, 1790 kcal of heat are released. We have to find out how many moles of C₃H₆O reacted in 177 mL. Considering the density of acetone is 0.788 g/mL and its molar mass is 58.08 g/mol, the moles of acetone are:

$177mL.\frac{0.788g}{mL} .\frac{1mol}{58.08g} =2.40mol$

The heat released when 2.40 moles of acetone burn is:

$2.40mol.\frac{(-1790kcal)}{1mol} =-4.30 \times 10^{3} kcal$