Question

Nail polish is primarily made of a compound called acetone (C₃H₆O; density = 0.788 g/mL; δH[[infinity]]combustion = -1790.00 kJ/mol).

Write the thermochemical equation for the combustion of acetone. (Hint: The water that forms is liquid.)

Answer 1

The thermochemical equation for the combustion of acetone, where the water produced is liquid, is 2 C3H6O(l) + 7 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -3580 kJ, accounting for two moles of acetone being combusted.

Step-by-step explanation:

The combustion of acetone (C3H6O) is a chemical reaction where acetone reacts with oxygen to produce carbon dioxide, water, and energy. The thermochemical equation for the combustion of acetone, where the water produced is in the liquid state, is as follows:

2 C3H6O(l) + 7 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -3580 kJ

It is essential to balance the chemical equation so that the number of atoms of each element is the same on both sides of the equation. The enthalpy change (ΔH) given in the question is for the combustion of one mole of acetone, but since two moles are being combusted in the balanced equation, the ΔH value is doubled to -3580 kJ to reflect this.

The thermochemical equation for the combustion of acetone (C3H6O) can be written as:

C3H6O(l) + 4O2(g) → 3CO2(g) + 3H2O(l)

In this reaction, acetone (a colorless liquid) reacts with oxygen gas to produce carbon dioxide gas and liquid water. The coefficients in the balanced equation indicate the stoichiometric ratio of each reactant and product.