Domanda del libro di testo
Balance each redox reaction occurring in basic aqueous solution. c. Cl2(g) → Cl–(aq) + ClO–(aq)
Ch.19 - Electrochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
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Capitolo 19, Problema 40c
Balance each redox reaction occurring in acidic aqueous solution. c. NO3–(aq) + Sn2+(aq) → Sn4+(aq) + NO(g)
Guida verificata passo dopo passo1
Identify the oxidation states of each element in the reactants and products. For NO3-, nitrogen is +5 and oxygen is -2. For Sn2+, tin is +2. In the products, for Sn4+, tin is +4, and for NO, nitrogen is +2.
Determine the changes in oxidation states to identify which elements are oxidized and which are reduced. Tin (Sn) is oxidized as its oxidation state increases from +2 to +4. Nitrogen (N) is reduced as its oxidation state decreases from +5 to +2.
Write the half-reactions for both oxidation and reduction. For oxidation: Sn2+ -> Sn4+ + 2e-. For reduction: NO3- + 4H+ + 3e- -> NO + 2H2O.
Balance the electrons in the half-reactions by multiplying the half-reactions by appropriate factors so that the number of electrons gained in the reduction half-reaction equals the number of electrons lost in the oxidation half-reaction. Multiply the oxidation half-reaction by 3 and the reduction half-reaction by 2.
Add the balanced half-reactions together and simplify to get the overall balanced equation in acidic solution: 3Sn2+ + 2NO3- + 8H+ -> 3Sn4+ + 2NO + 4H2O.
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Redox Reactions
Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between two species. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the oxidation states of the elements involved is crucial for identifying which species undergo these changes.
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03:12
Identifying Redox 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: one for oxidation and one for reduction. In acidic solutions, hydrogen ions (H+) and water (H2O) are typically added to balance the equation, along with electrons to balance the charge.
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01:04Balancing Basic Redox Reactions
Acidic Aqueous Solutions
In acidic aqueous solutions, the presence of H+ ions influences the behavior of the reactants and products. The pH level can affect the solubility and reactivity of certain species. When balancing redox reactions in such environments, it is essential to account for these ions, as they can participate in the reaction and affect the overall stoichiometry.
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Percorso guidato
01:11Types of Aqueous Solutions
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