Textbook Question
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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Ch.20 - Electrochemistry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 20, Problem 24a,b,c,d
Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) Mo3+(aq) → Mo(s) (acidic solution) (b) H2SO3(aq) → SO42-(aq) (acidic solution) (c) NO3-(aq) → NO(g) (acidic solution) (d) O2(g) → H2O(l) (acidic solution)
Verified step by step guidance1
Identify the oxidation states of sulfur in H_2SO_3 and SO_4^{2-}.
Determine the change in oxidation state to identify if it is oxidation or reduction.
Balance the sulfur atoms on both sides of the equation.
Balance the oxygen atoms by adding H_2O molecules to the side that needs more oxygen.
Balance the hydrogen atoms by adding H^+ ions to the side that needs more hydrogen.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Half-Reactions
Half-reactions are the individual oxidation or reduction processes that occur in a redox reaction. They represent the transfer of electrons, with oxidation involving the loss of electrons and reduction involving the gain of electrons. Balancing half-reactions is essential for understanding the overall redox process and ensuring that the number of electrons lost equals the number gained.
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First-Order Half-Life
Oxidation and Reduction
Oxidation is defined as the process where a substance loses electrons, resulting in an increase in oxidation state, while reduction is the gain of electrons, leading to a decrease in oxidation state. In redox reactions, one species is oxidized and another is reduced, and identifying these processes is crucial for balancing chemical equations and understanding reaction mechanisms.
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01:53Oxidation and Reduction Reactions
Balancing Redox Reactions in Acidic Solution
When balancing redox reactions in acidic solutions, it is important to account for hydrogen ions (H+) and water (H2O) to ensure mass and charge balance. The steps typically involve separating the half-reactions, balancing the atoms other than O and H, then balancing O with H2O and H with H+. Finally, the charges are balanced by adding electrons, which helps in determining the overall balanced equation.
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Related Practice
Textbook Question
Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (a) Sn2+(aq) → Sn4+(aq) (acidic solution) (b) TiO2(s) → Ti2+(aq) (acidic solution) (c) ClO3-(aq) → Cl-(aq) (acidic solution) (d) N2(g) → NH4+(aq) (acidic solution)
Textbook Question
Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (g) Cr(OH)3(s) → CrO42-(aq) (basic solution)
Textbook Question
Hydrazine (N2H4) and dinitrogen tetroxide (N2O4) form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (c) Which substance serves as the reducing agent and which as the oxidizing agent?
Textbook Question
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)
Textbook Question
Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (f) SO32-1aq2 ¡ SO42-1aq2 (basic solution)
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