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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Ch.20 - Electrochemistry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 20, Problema 28
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)
Guida verificata passo dopo passo1
Step 1: Identify the oxidation states of each element in the reactants and products for each equation to determine which elements are oxidized and reduced.
Step 2: Write the half-reactions for the oxidation and reduction processes separately for each equation.
Step 3: Balance each half-reaction for mass and charge. In acidic solutions, add H2O to balance oxygen and H+ to balance hydrogen. In basic solutions, add OH- to balance both hydrogen and oxygen.
Step 4: Multiply each half-reaction by appropriate coefficients so that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.
Step 5: Add the balanced half-reactions together, canceling out electrons and any other species that appear on both sides, to obtain the balanced overall equation. Identify the oxidizing agent (species that is reduced) and the reducing agent (species that is oxidized).
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Redox Reactions
Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between species. In these reactions, one substance is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the electron transfer is crucial for identifying the oxidizing and reducing agents in a reaction.
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Percorso guidato
03:12
Identifying Redox Reactions
Balancing Chemical Equations
Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. This process often involves adjusting coefficients and may require separate balancing of oxidation and reduction half-reactions in redox processes.
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Percorso guidato
01:32Balancing Chemical Equations
Oxidizing and Reducing Agents
The oxidizing agent is the species that gets reduced by gaining electrons, while the reducing agent is the species that gets oxidized by losing electrons. Identifying these agents is essential in redox reactions, as they play a key role in determining the direction of electron flow and the overall reaction mechanism.
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Percorso guidato
01:01Oxidizing and Reducing Agents
Pratica correlata
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 equations, and identify the oxidizing and reducing agents: MnO4-(aq) + Br-(aq) → MnO2(s) + BrO3-(aq) (basic solution)
703
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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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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. S(s) + HNO3(aq) → H2SO3(aq) + N2O(g) (acidic solution)
b. BrO3-(aq) + N2H4(g) → Br-(aq) + N2(g) (acidic solution)
c. H2O2(aq) + ClO2(aq) → ClO20(aq) _ O2(g) (basic solution)