Question

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.

Answer 1

Answer:

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 = $\frac{mass}{molarmass}=\frac{139.48}{58} =2.4 mol$

The energy produced = moles present X enthalpy of reaction

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