Domanda del libro di testo
A cell has a standard cell potential of +0.177 V at 298 K. What is the value of the equilibrium constant for the reaction
(a) if n = 1?
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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
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Capitolo 20, Problema 62
At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the reaction is 5.5 × 105. What is the value of n for the reaction?
Guida verificata passo dopo passo1
Identify the relationship between the standard cell potential (E°), the equilibrium constant (K), and the number of moles of electrons transferred (n) using the Nernst equation at equilibrium: E° = (RT/nF)ln(K).
Since the temperature is 298 K, use the simplified form of the Nernst equation: E° = (0.0257 V/n)ln(K).
Substitute the given values into the equation: 0.17 V = (0.0257 V/n)ln(5.5 × 10^5).
Solve for n by isolating it on one side of the equation: n = (0.0257 V/0.17 V)ln(5.5 × 10^5).
Calculate the natural logarithm of the equilibrium constant and then solve for n.
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Nernst Equation
The Nernst Equation relates the cell potential of an electrochemical reaction to the concentrations of the reactants and products. It is expressed as E = E° - (RT/nF)ln(Q), where E is the cell potential, E° is the standard cell potential, R is the universal 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.
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01:17
The Nernst Equation
Standard Cell Potential (E°)
The standard cell potential (E°) is the voltage measured under standard conditions (1 M concentration, 1 atm pressure, and 25°C) for a galvanic cell. It indicates the tendency of a chemical reaction to occur spontaneously; a positive E° suggests a spontaneous reaction, while a negative E° indicates non-spontaneity.
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01:27Standard Cell Potential
Equilibrium Constant (K)
The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It is related to the standard cell potential through the equation ΔG° = -nFE°, where ΔG° is the change in Gibbs free energy. A larger K value indicates a greater tendency for the reaction to favor products at equilibrium.
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01:14Equilibrium Constant K