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What reaction can occur, if any, when the following experiments are carried out under standard-state conditions? (c) A silver wire is immersed in an aqueous solution of NiCl2.
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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 84
The standard potential for the following galvanic cell is 0.40 V: (Europium, Eu, is one of the lanthanide elements.) Use the data in Table 19.1 to calculate the standard reduction potential for Eu3+/Eu2+ half-cell.
Guida verificata passo dopo passo1
Identify the overall cell reaction and the half-reactions involved in the galvanic cell.
Use the standard cell potential formula: E°_cell = E°_cathode - E°_anode.
Determine which half-reaction corresponds to the cathode and which to the anode using the given standard cell potential.
Look up the standard reduction potential for the other half-cell from Table 19.1.
Rearrange the standard cell potential formula to solve for the unknown standard reduction potential of the Eu3+/Eu2+ half-cell.
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Galvanic Cells
Galvanic cells, also known as voltaic cells, are electrochemical cells that convert chemical energy into electrical energy through spontaneous redox reactions. In these cells, oxidation occurs at the anode and reduction at the cathode, generating a flow of electrons that can be harnessed for electrical power. The standard cell potential is determined by the difference in standard reduction potentials of the half-reactions involved.
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01:08
The Galvanic Cell
Standard Reduction Potential
Standard reduction potential (E°) is a measure of the tendency of a chemical species to gain electrons and be reduced, expressed in volts. Each half-reaction has a specific E° value, which is determined under standard conditions (1 M concentration, 1 atm pressure, and 25°C). The more positive the E° value, the greater the species' ability to be reduced, making it a crucial factor in calculating the overall cell potential.
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01:10Standard Reduction Potentials
Nernst Equation
The Nernst equation relates the cell potential to the concentrations of the reactants and products in a redox reaction. It allows for the calculation of the cell potential under non-standard conditions and can be rearranged to find standard potentials when the overall cell potential and one half-cell potential are known. This equation is essential for determining the standard reduction potential of the Eu3+/Eu2+ half-cell in the context of the given galvanic cell.
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01:17The Nernst Equation
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