Domanda del libro di testo
A mercury battery uses the following electrode half-reactions: (c) What is the effect on the cell voltage of a tenfold change in the concentration of KOH in the electrolyte? Explain..
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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 122
For a lead storage battery: (a) Sketch one cell that shows the anode, cathode, electrolyte, direction of electron and ion flow, and sign of the electrodes. (b) Write the anode, cathode, and overall cell reactions. (c) Calculate the equilibrium constant for the cell reaction (E° = 1.924 V). (d) What is the cell voltage when the cell reaction reaches equilibrium?
Guida verificata passo dopo passo1
Step 1: Understand the components of a lead storage battery. The anode is made of lead (Pb), the cathode is lead dioxide (PbO2), and the electrolyte is sulfuric acid (H2SO4). Electrons flow from the anode to the cathode through an external circuit, while ions move through the electrolyte.
Step 2: Write the half-reactions for the anode and cathode. At the anode, lead is oxidized: \( \text{Pb} \rightarrow \text{Pb}^{2+} + 2\text{e}^- \). At the cathode, lead dioxide is reduced: \( \text{PbO}_2 + 4\text{H}^+ + 2\text{e}^- \rightarrow \text{Pb}^{2+} + 2\text{H}_2\text{O} \).
Step 3: Combine the half-reactions to write the overall cell reaction. Ensure that the electrons cancel out: \( \text{Pb} + \text{PbO}_2 + 4\text{H}^+ \rightarrow 2\text{Pb}^{2+} + 2\text{H}_2\text{O} \).
Step 4: Use the Nernst equation to calculate the equilibrium constant \( K \) for the cell reaction. The equation is \( E^\circ = \frac{RT}{nF} \ln K \), where \( E^\circ \) 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, and \( F \) is Faraday's constant.
Step 5: Determine the cell voltage at equilibrium. At equilibrium, the cell voltage is zero because the forward and reverse reactions occur at the same rate, and there is no net electron flow.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Electrochemical Cells
Electrochemical cells consist of two electrodes (anode and cathode) immersed in an electrolyte, facilitating redox reactions. The anode is where oxidation occurs, releasing electrons, while the cathode is where reduction takes place, accepting electrons. Understanding the flow of electrons and ions is crucial for analyzing the cell's operation and sketching its components accurately.
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02:46
Electrochemical Cells
Cell Reactions and Standard Electrode Potentials
Cell reactions in electrochemical cells involve the transfer of electrons between the anode and cathode, which can be represented by half-reactions. The standard electrode potential (E°) quantifies the tendency of a species to gain electrons, influencing the overall cell reaction. Writing the anode and cathode reactions is essential for calculating the overall cell reaction and its equilibrium constant.
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01:27Standard Cell Potential
Equilibrium Constant and Cell Voltage
The equilibrium constant (K) for a cell reaction can be calculated using the Nernst equation, which relates the standard cell potential (E°) to the concentrations of reactants and products at equilibrium. At equilibrium, the cell voltage drops to zero, indicating no net reaction occurs. Understanding how to calculate K and interpret cell voltage is vital for predicting the behavior of the electrochemical cell under different conditions.
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02:38Cell Potential and Equilibrium
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