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.

-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:

The heat released when 2.40 moles of acetone burn is:

it is a good conductor

explanation: