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Chapter 12: Problem 177

Carbon dioxide, \(\mathrm{CO}_{2}\), is a compound of carbon and oxygen. Does this mean that a sample of pure carbon dioxide can be considered to be a solution of carbon dissolved in oxygen? Explain your answer.

Short Answer

Expert verified
A sample of pure carbon dioxide cannot be considered a solution of carbon dissolved in oxygen. This is because carbon dioxide (CO2) is a compound formed by the chemical bonding of carbon and oxygen, creating a new substance with distinct properties. In a solution, the chemical properties of the solute and solvent remain unchanged, which is not the case for CO2. Hence, CO2 is a compound, not a solution.

Step by step solution

01

Understanding Compounds

A compound is a substance formed when two or more elements chemically bond together. In this case, the chemical properties of the elements change, forming a new substance with distinct properties. Carbon dioxide (CO2) is a compound since carbon and oxygen chemically bond together.
02

Understanding Solutions

A solution is a homogeneous mixture of two or more substances. In a solution, the solute is the substance that gets dissolved, and the solvent is the substance that does the dissolving. The chemical properties of the solute and the solvent remain unchanged in a solution.
03

Analyzing Carbon Dioxide (CO2)

Now that we understand what compounds and solutions are, we can analyze CO2. Carbon dioxide is formed when a carbon atom (C) chemically bonds with two oxygen atoms (O). As a result, the chemical properties of carbon and oxygen change, and a new substance with distinct properties is formed. Therefore, CO2 is a compound, not a solution.
04

Conclusion

Carbon dioxide (CO2) is not a solution of carbon dissolved in oxygen but instead, a compound formed by the chemical bonding of carbon and oxygen. The chemical properties of carbon and oxygen change during this bonding process, creating a new substance with different properties than its constituent elements.

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Most popular questions from this chapter

A \(25.00 \mathrm{~mL}\) sample of aqueous sulfuric acid of unknown concentration is neutralized by \(27.55\) \(\mathrm{mL}\) of \(1.0002 \mathrm{M} \mathrm{NaOH}(a q)\) (a) Write a net ionic equation for this acid-base neutralization reaction. (b) How many moles of \(\mathrm{NaOH}\) did it take for the neutralization? (c) How many moles of sulfuric acid were neutralized? (d) What is the molar concentration of the sulfuric acid?

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