Consider the thermochemical equation for the combustion of acetone (c3h6o), the main ingredient in nail polish remover: c3h6o(l)+4 o2(g)→3 co2(g)+3 h2o(g)δh°rxn=−1790 kj if a bottle of nail polish remover contains 177 ml of acetone, how much heat is released by its complete combustion? the density of acetone is 0.788 g/ml.

the energy produced or released = 2.4 X (-1790) = -4296 kJ

Explanation:

In the given question the heat of combustion is given as H°rxn = −1790 kJ

Thus when one mole of acetone undergoes complete combustion, it gives this much of energy.

The volume of acetone present in nail polish remover = 177 mL

The density of acetone = 0.788 g/mL

The mass of acetone present in nail polish remover = density X volume

the mass of acetone = 0.788 X 177 = 139.48 grams

the moles of acetone present =

The energy produced = moles present X enthalpy of reaction

the energy produced or released = 2.4 X (-1790) = -4296 kJ