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Balancing a chemical equation is like solving a puzzle. The goal is to have the same number of each type of atom on both sides of the equation. This ensures the law of conservation of mass is satisfied, meaning that mass is neither created nor destroyed in a chemical reaction. For example, in the combustion of acetone, represented by the chemical formula \( \text{C}_3\text{H}_6\text{O} \), we start with an unbalanced equation:
\[ \text{C}_3\text{H}_6\text{O}(l) + \text{O}_2(g) \rightarrow \text{CO}_2(g) + \text{H}_2\text{O}(l) \]
To balance it:

• Start with carbon: Acetone has 3 carbon atoms, so we need 3 \( \text{CO}_2 \) molecules.
• Next, balance hydrogen: There are 6 hydrogen atoms in acetone, requiring 3 \( \text{H}_2\text{O} \) molecules.
• Finally, balance oxygen: Check the number of oxygen atoms needed, which ends up requiring 4 \( \text{O}_2 \) molecules.

Thus, the balanced equation for the combustion of acetone is:\[\text{C}_3\text{H}_6\text{O}(l) + 4\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 3\text{H}_2\text{O}(l)\]

Acetone, commonly known as nail polish remover, undergoes combustion, a process that involves burning in the presence of oxygen. This reaction is an example of a chemical reaction where energy is released, usually in the form of heat and light. Combustion of organic compounds like acetone, which contain carbon, hydrogen, and oxygen, typically results in the formation of carbon dioxide and water.
In practical terms, acetone combusts according to the equation:
\[\text{C}_3\text{H}_6\text{O}(l) + 4\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 3\text{H}_2\text{O}(l)\]
This reaction illustrates complete combustion, meaning acetone is fully converted into \( \text{CO}_2 \) and \( \text{H}_2\text{O} \) without any leftover acetone. It's important to have enough oxygen to ensure complete combustion, preventing the formation of carbon monoxide or other byproducts.

Oxygen is a critical reactant in combustion reactions. It pairs with hydrocarbons, substances made of hydrogen and carbon, or compounds containing carbon, hydrogen, and oxygen to sustain the reaction. Without sufficient oxygen, combustion cannot occur. This is why oxygen is always involved in burning processes, such as the combustion of acetone.
In the combustion of acetone, \( \text{O}_2 \) molecules are needed to break the bonds in the acetone molecule and rearrange its atoms to form new compounds:

• The chemical equation shows that 4 molecules of \( \text{O}_2 \) are necessary to react with 1 molecule of acetone.
• The presence of oxygen ensures carbon is converted into carbon dioxide and hydrogen into water, completing the reaction.

Without enough oxygen, incomplete combustion might occur, leading to lower energy output and the potential production of harmful substances like carbon monoxide.

The combustion products of any hydrocarbon or oxygen-containing hydrocarbon like acetone are primarily carbon dioxide and water. These products result from the chemical transformation that occurs during combustion. Each carbon atom in the fuel combines with oxygen to form \( \text{CO}_2 \), while each pair of hydrogen atoms combines with oxygen to form \( \text{H}_2\text{O} \).
In the case of acetone, the balanced chemical reaction tells us:

• 3 molecules of \( \text{CO}_2 \) are produced from the 3 carbon atoms in acetone.
• 3 molecules of \( \text{H}_2\text{O} \) result from the 6 hydrogen atoms.

This conversion is efficient and maximizes energy release, which is why \( \text{CO}_2 \) and \( \text{H}_2\text{O} \) are the hallmark products of any complete combustion process.