Domanda del libro di testo
The following cell reactions occur spontaneously: (a) Arrange the following reduction half-reactions in order of decreasing tendency to occur:
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Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 19, Problema 80a
Use the data in Appendix D to predict whether the following reactions can occur under standard-state conditions. (a) Oxidation of Sn2+(aq) by Br2(aq)
Guida verificata passo dopo passo1
Identify the half-reactions involved in the oxidation of \( \text{Sn}^{2+} \) by \( \text{Br}_2 \).
Write the reduction half-reaction for \( \text{Br}_2 \) and the oxidation half-reaction for \( \text{Sn}^{2+} \).
Use Appendix D to find the standard reduction potentials \( E^0 \) for each half-reaction.
Calculate the standard cell potential \( E^0_{\text{cell}} \) by subtracting the oxidation potential from the reduction potential.
Determine if the reaction is spontaneous under standard conditions by checking if \( E^0_{\text{cell}} > 0 \).
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Standard-State Conditions
Standard-state conditions refer to a set of specific conditions used to measure the properties of substances. These conditions typically include a temperature of 25°C (298 K), a pressure of 1 atm, and concentrations of 1 M for solutions. Understanding these conditions is crucial for predicting the feasibility of chemical reactions, as they provide a baseline for comparing thermodynamic data.
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01:10
Standard Reduction Potentials
Oxidation-Reduction Reactions
Oxidation-reduction (redox) reactions involve the transfer of electrons between species, resulting in changes in oxidation states. In the given reaction, Sn<sup>2+</sup> is oxidized to Sn<sup>4+</sup>, while Br<sub>2</sub> is reduced to Br<sup>-</sup>. Identifying the oxidizing and reducing agents is essential for predicting whether the reaction can occur spontaneously under standard-state conditions.
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01:53Oxidation and Reduction Reactions
Electrochemical Cell Potential
The electrochemical cell potential, or standard cell potential (E°), is a measure of the driving force behind a redox reaction. It can be calculated using standard reduction potentials from tables. A positive E° indicates that the reaction is spontaneous under standard-state conditions, while a negative E° suggests it is non-spontaneous. This concept is vital for predicting the feasibility of the oxidation of Sn<sup>2+</sup> by Br<sub>2</sub>.
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02:46Electrochemical Cells
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