Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 88b

Chapter 3, Problem 88b

If 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol C6H6 are completely combusted in oxygen, which one produces the least? Explain.

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Identify the chemical formulas for each compound: CH3CH2CH2COOH (butanoic acid), C4H10 (butane), and C6H6 (benzene).

Write the balanced chemical equations for the complete combustion of each compound: \( \text{CH}_3\text{CH}_2\text{CH}_2\text{COOH} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \), \( \text{C}_4\text{H}_{10} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \), \( \text{C}_6\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \).

Determine the number of moles of \( \text{CO}_2 \) produced per mole of each compound by using the stoichiometry from the balanced equations.

Calculate the total moles of \( \text{CO}_2 \) produced for 2.0 moles of each compound by multiplying the moles of \( \text{CO}_2 \) per mole of compound by 2.0.

Compare the total moles of \( \text{CO}_2 \) produced by each compound to determine which one produces the least amount of \( \text{CO}_2 \).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Combustion Reaction

A combustion reaction is a chemical process in which a substance reacts with oxygen to produce heat and light. Typically, hydrocarbons combust to form carbon dioxide and water. The amount of energy released during combustion depends on the structure of the hydrocarbon and the number of carbon and hydrogen atoms present.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the moles of products formed from a given amount of reactants. In this case, knowing the stoichiometric coefficients for the combustion of each hydrocarbon will help us compare the total moles of carbon dioxide produced.

Energy Content of Fuels

The energy content of fuels, often measured in kilojoules per mole, indicates how much energy is released during combustion. Different hydrocarbons have varying energy contents based on their molecular structure. By comparing the energy released per mole of each compound during combustion, we can determine which fuel produces the least energy and, consequently, the least amount of products.

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