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Ch.6 - Thermochemistry
All textbooksTro 4th EditionCh.6 - ThermochemistryProblem 59
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Chapter 6, Problem 59

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.

Verified step by step guidance
1
<Calculate the mass of acetone using its volume and density: mass = volume \times density.>
<Convert the mass of acetone to moles using its molar mass: moles = \frac{mass}{molar\ mass}.>
<Use the stoichiometry of the reaction to determine the heat released: \Delta H_{rxn} is given per mole of acetone.>
<Multiply the moles of acetone by the \Delta H_{rxn} to find the total heat released.>
<Ensure the units are consistent and the final answer is in kilojoules (kJ).>
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Related Practice
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