Domanda del libro di testo
Consider a galvanic cell that uses the reaction Calculate the potential at 25 °C for a cell that has the following ion concentrations: [Ag+] = 0.010M, [Ni2+] = 0.100M.
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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 97
A galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with a CuSO4 solu-tion. If the measured cell potential at 25 °C is 0.67 V, what is the concentration of Cu2+ in the CuSO4 solution?
Guida verificata passo dopo passo1
Identify the half-reactions for the galvanic cell: Fe(s) \(\rightarrow\) Fe^{2+}(aq) + 2e^- and Cu^{2+}(aq) + 2e^- \(\rightarrow\) Cu(s).
Write the overall cell reaction by combining the half-reactions: Fe(s) + Cu^{2+}(aq) \(\rightarrow\) Fe^{2+}(aq) + Cu(s).
Use the Nernst equation to relate the cell potential to the concentrations: E_{cell} = E^\(\circ\)_{cell} - \(\frac{RT}{nF}\) \(\ln\) Q, where Q is the reaction quotient.
Calculate the standard cell potential, E^\(\circ\)_{cell}, using standard reduction potentials: E^\(\circ\)_{cell} = E^\(\circ\)_{Cu^{2+}/Cu} - E^\(\circ\)_{Fe^{2+}/Fe}.
Solve for the concentration of Cu^{2+} using the Nernst equation and the given cell potential, 0.67 V, by substituting known values and solving for the unknown concentration.
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Galvanic Cell
A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two electrodes, an anode and a cathode, immersed in electrolyte solutions. The flow of electrons from the anode to the cathode generates an electric current, and the cell potential is determined by the difference in reduction potentials of the two half-reactions.
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01:08
The Galvanic Cell
Nernst Equation
The Nernst equation relates the cell potential to the concentrations of the reactants and products in an electrochemical reaction. It is expressed as E = E° - (RT/nF) ln(Q), where E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is Faraday's constant, and Q is the reaction quotient. This equation allows for the calculation of cell potential under non-standard conditions.
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01:17The Nernst Equation
Reaction Quotient (Q)
The reaction quotient (Q) is a measure of the relative concentrations of reactants and products in a chemical reaction at a given moment. It is calculated using the formula Q = [products]/[reactants], where the concentrations are raised to the power of their coefficients in the balanced equation. In the context of a galvanic cell, Q helps determine the direction of the reaction and the cell potential, especially when concentrations deviate from standard conditions.
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00:49Reaction Quotient Q
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