Consider the thermochemical equation for the combustion of acetone (C3 H6 O), the main ingredien

step 1 In this question we're going to be applying the geometry and some heat equations to determine th

Consider the thermochemical equation for the combustion of...

Consider the thermochemical equation for the combustion of acetone $\left(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\right)$, the main ingredient in nail polish remover. $\begin{aligned} \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l)+4 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g) \\ \Delta H_{\mathrm{ran}}^{\circ} &=-1790 \mathrm{~kJ} \end{aligned}$ If a bottle of nail polish remover contains $177 \mathrm{~mL}$ of acetone, how much heat is released by its complete combustion? The density of acetone is $0.788 \mathrm{~g} / \mathrm{mL}$.

Consider the thermochemical equation for the combustion of acetone $\left(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\right)$, the main ingredient in nail polish remover.
$\begin{aligned} \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l)+4 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(g) \\ \Delta H_{\mathrm{ran}}^{\circ} &=-1790 \mathrm{~kJ} \end{aligned}$
If a bottle of nail polish remover contains $177 \mathrm{~mL}$ of acetone, how much heat is released by its complete combustion? The density of acetone is $0.788 \mathrm{~g} / \mathrm{mL}$.

Key Concepts

Density Conversion

Density conversion is a method used to relate the mass of a substance to its volume through the density value. In practical scenarios, such as determining how much of a liquid reactant is available for a reaction, knowing the substance's density allows for the conversion of volume (in mL or L) to mass (in grams), which can then be used in further quantitative analyses like stoichiometric calculations.

Molar Mass Calculation

Molar mass calculation involves determining the mass of one mole of a given compound. By using the molecular formula of a substance, the individual atomic masses are summed to yield the compound’s molar mass, typically expressed in grams per mole. This concept is essential for converting between the mass of a substance and the number of moles, linking laboratory measurements to chemical reaction quantities.

Thermochemistry

Thermochemistry deals with the study of the heat energy involved in chemical reactions and changes of state. It involves understanding how energy is absorbed or released during reactions, notably through the concept of enthalpy change. In combustion reactions, for instance, the heat released is quantified using thermochemical equations where the enthalpy change (?H) is given per mole of reactant or product, allowing for calculations on a macroscopic scale.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It involves interpreting balanced chemical equations to determine how many moles of each substance participate in the reaction, which is crucial when calculating the total energy released or consumed. This concept enables the linking of molecular-scale reactions to measurable amounts of substances.

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