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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.20 - ElectrochemistryProblema 27c
Capitolo 20, Problema 27c

Complete and balance the following equations, and identify the oxidizing and reducing agents: MnO4-(aq) + Br-(aq) → MnO2(s) + BrO3-(aq) (basic solution)

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Step 1: Separate the reaction into two half-reactions, one for oxidation and one for reduction. Identify the species being oxidized and reduced.
Step 2: Balance each half-reaction for mass and charge. Start by balancing all elements except for oxygen and hydrogen. Then, balance oxygen atoms by adding H2O molecules, and balance hydrogen atoms by adding OH- ions (since the solution is basic). Finally, balance the charges by adding electrons.
Step 3: Multiply each half-reaction by an appropriate coefficient so that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.
Step 4: Add the balanced half-reactions together, canceling out any species that appear on both sides of the equation, such as electrons, water, or hydroxide ions.
Step 5: Identify the oxidizing agent (the species that is reduced) and the reducing agent (the species that is oxidized) in the balanced equation.

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Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In these reactions, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Understanding these processes is crucial for identifying the oxidizing and reducing agents in a chemical equation.
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Oxidation and Reduction Reactions

Balancing Redox Reactions

Balancing redox reactions requires ensuring that both mass and charge are conserved. This often involves separating the reaction into half-reactions for oxidation and reduction, balancing each half for atoms and charge, and then combining them. In basic solutions, hydroxide ions (OH-) may be added to balance the reaction, which is essential for achieving the correct stoichiometry.
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Balancing Basic Redox Reactions

Identifying Oxidizing and Reducing Agents

The oxidizing agent is the species that is reduced (gains electrons) during the reaction, while the reducing agent is the species that is oxidized (loses electrons). Identifying these agents is key to understanding the dynamics of the reaction and predicting the products formed. In the given equation, recognizing the changes in oxidation states helps in pinpointing these agents.
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Oxidizing and Reducing Agents
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Domanda del libro di testo

Complete and balance the following equations, and identify the oxidizing and reducing agents:


a. MnO4−(𝑎𝑞)+CH3OH(𝑎𝑞)⟶Mn2+(𝑎𝑞)+HCOOH(𝑎𝑞)(acidic solution)

b. As2O3(𝑠)+NO3−(𝑎𝑞)⟶H3AsO4(𝑎𝑞)+N2O3(𝑎𝑞)(acidic solution)

c. Pb(OH)42−(𝑎𝑞)+ClO−(𝑎𝑞)⟶PbO2(𝑠)+Cl−(𝑎𝑞)(basic solution)

Domanda del libro di testo

Complete and balance the following equations, and identify the oxidizing and reducing agents: As2O3(s) + NO3-(aq) → H3AsO4(aq) + N2O3(aq) (acidic solution)

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Domanda del libro di testo

Complete and balance the following equations, and identify the oxidizing and reducing agents: (a) Cr2O72-(aq) + I-(aq) → Cr3+(aq) + IO3-(aq) (acidic solution) (b) MnO4-(aq) + CH3O(1aq) → Mn2+(aq) + HCOOH(aq) (acidic solution) (c) I2(s) + OCl-(aq) → IO3-(aq) + Cl-(aq) (acidic solution)

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Domanda del libro di testo

Complete and balance the following half-reactions in basic solution. In each case, indicate whether the half-reaction is an oxidation or a reduction. c. Cr(OH)3(𝑠)⟶CrO42−(𝑎𝑞)

Domanda del libro di testo

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H2O2, have an atypical oxidation state.) (a) NO2-(aq) + Cr2O72-(aq) → Cr3+(aq) + NO3-(aq) (acidic solution) (b) S(s) + HNO3(aq) → H2SO3(aq) + N2O(g) (acidic solution) (c) Cr2O72- (aq) + CH3OH(aq) → HCOOH(aq) + Cr3+(aq) (acidic solution) (d) BrO3-(aq) + N2H4(g) → Br-(aq) + N2(g) (acidic solution)

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Domanda del libro di testo

Complete and balance the following half-reactions in acidic solution. In each case indicate whether the half-reaction is an oxidation or a reduction. b. H2SO3(𝑎𝑞)⟶SO42−(𝑎𝑞)

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