Textbook Question
Determine whether each of the following chemical equations is balanced or not balanced:
d.
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Ch.7 Chemical Quantities and Reactions
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353
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Table of contents
- Ch.1 Chemistry in Our Lives11
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy54
- Ch.4 Atoms and Elements51
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions41
- Ch.8 Gases29
- Ch.9 Solutions51
- Ch.10 Acids and Bases and Equilibrium65
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons78
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones83
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides90
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis83
- Ch.18 Metabolic Pathways and ATP Production67
Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353Not the one you use?Change textbook
Chapter 7, Problem 45c
Identify each of the following as an oxidation or a reduction:
c. Cr3+(aq) + 3e– → Cr(s)
Verified step by step guidance1
Step 1: Recall the definitions of oxidation and reduction. Oxidation is the loss of electrons, while reduction is the gain of electrons. A helpful mnemonic is 'OIL RIG' (Oxidation Is Loss, Reduction Is Gain).
Step 2: Analyze the given chemical equation: Cr³⁺(aq) + 3e⁻ → Cr(s). Notice that the chromium ion (Cr³⁺) is reacting with three electrons (3e⁻).
Step 3: Determine if electrons are being gained or lost. In this case, Cr³⁺ is gaining three electrons to form Cr(s).
Step 4: Conclude that the gain of electrons corresponds to a reduction process. Therefore, this reaction represents a reduction.
Step 5: Summarize the result: The reaction Cr³⁺(aq) + 3e⁻ → Cr(s) is a reduction because the chromium ion gains electrons to form a neutral chromium atom.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidation and Reduction
Oxidation and reduction are chemical processes that involve the transfer of electrons between species. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. These processes are always coupled; when one species is oxidized, another must be reduced. Understanding these definitions is crucial for identifying the nature of chemical reactions.
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Half-Reaction Method
The half-reaction method is a way to balance redox reactions by separating the oxidation and reduction processes. Each half-reaction shows either the loss or gain of electrons, making it easier to analyze the changes in oxidation states. This method is particularly useful in identifying which species is oxidized and which is reduced in a given reaction.
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Oxidation States
Oxidation states (or numbers) indicate the degree of oxidation of an atom in a compound. They help in determining how many electrons are lost or gained during a reaction. In the given reaction, the oxidation state of chromium changes from +3 in Cr³⁺ to 0 in Cr(s), indicating that it is being reduced. Understanding oxidation states is essential for identifying the nature of the reaction.
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Related Practice
Textbook Question
Balance each of the following chemical equations:
c. Sb2S3(s) + HCl(aq) → SbCl3(aq) + H2S(g)
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Textbook Question
Balance each of the following chemical equations:
d. Al(s) + HCl(aq) → H2(g) + AlCl3(aq)
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Textbook Question
In the mitochondria of human cells, energy is provided by the oxidation and reduction reactions of the iron ions in the cytochromes in electron transport. Identify each of the following as an oxidation or a reduction:
a. Fe3+ + e– → Fe2+
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Textbook Question
The chemical reaction of hydrogen with oxygen produces water.
2 H2(g) + O2(g) → 2 H2O(g)
c. How many moles of H2O form when 2.5 moles of O2 reacts?
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Textbook Question
Why do chemical reactions require energy of activation?
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