(c) What is the sum of the coefficients in the balanced chemical equation for the combustion of one mole of acetone, C3H6O1l2, in air?

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1. Write the unbalanced chemical equation for the combustion of acetone: \( \text{C}_3\text{H}_6\text{O}_{(l)} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \).
2. Balance the carbon atoms by ensuring there are 3 \( \text{CO}_2 \) molecules on the product side: \( \text{C}_3\text{H}_6\text{O}_{(l)} + \text{O}_2 \rightarrow 3\text{CO}_2 + \text{H}_2\text{O} \).
3. Balance the hydrogen atoms by ensuring there are 3 \( \text{H}_2\text{O} \) molecules on the product side: \( \text{C}_3\text{H}_6\text{O}_{(l)} + \text{O}_2 \rightarrow 3\text{CO}_2 + 3\text{H}_2\text{O} \).
4. Balance the oxygen atoms by adjusting the \( \text{O}_2 \) molecules on the reactant side. Count the total oxygen atoms needed on the product side and adjust accordingly.
5. Sum all the coefficients in the balanced equation, including the coefficient for \( \text{O}_2 \), to find the total sum.

Key Concepts

Combustion Reaction

A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, producing heat and light. In organic compounds, this typically involves the reaction of hydrocarbons with oxygen to produce carbon dioxide and water. Understanding the general form of combustion reactions is essential for balancing the equation correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is achieved by adjusting the coefficients in front of the reactants and products. A balanced equation reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.

Coefficients in Chemical Equations

Coefficients are the numbers placed in front of the chemical formulas in a balanced equation to indicate the relative amounts of each substance involved in the reaction. The sum of the coefficients provides insight into the stoichiometry of the reaction, which is crucial for understanding the proportions of reactants and products in a chemical process.