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A friend wants you to invest in a new battery she has designed that produces 24 V in a single voltaic cell. Why should you be wary of investing in such a battery?
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Ch.19 - Electrochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 19, Problema 111
The cell potential of this electrochemical cell depends on the pH of the solution in the anode half-cell. Pt(s) | H2(g, 1 atm) | H+(aq, ? M) || Cu2+(aq, 1.0 M) | Cu(s) What is the pH of the solution if Ecell is 355 mV?
Guida verificata passo dopo passo1
Identify the half-reactions for the electrochemical cell. The anode half-reaction involves hydrogen: \( \text{H}_2(g) \rightarrow 2\text{H}^+(aq) + 2e^- \). The cathode half-reaction involves copper: \( \text{Cu}^{2+}(aq) + 2e^- \rightarrow \text{Cu}(s) \).
Write the Nernst equation for the cell potential: \( E_{cell} = E^\circ_{cell} - \frac{RT}{nF} \ln Q \), where \( Q \) is the reaction quotient.
Calculate the standard cell potential \( E^\circ_{cell} \) using standard reduction potentials: \( E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} \). Use standard reduction potentials for \( \text{Cu}^{2+}/\text{Cu} \) and \( \text{H}^+/\text{H}_2 \).
Express the reaction quotient \( Q \) in terms of concentrations: \( Q = \frac{[\text{H}^+]^2}{[\text{Cu}^{2+}]} \). Given \([\text{Cu}^{2+}] = 1.0 \text{ M}\), simplify \( Q \) to \( [\text{H}^+]^2 \).
Rearrange the Nernst equation to solve for \([\text{H}^+]\), and then calculate the pH using \( \text{pH} = -\log[\text{H}^+] \).
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Concetti chiave
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Nernst Equation
The Nernst Equation relates the cell potential (E) of an electrochemical cell to the concentrations of the reactants and products. 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 us to calculate the effect of concentration changes on the cell potential.
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Percorso guidato
01:17
The Nernst Equation
pH and Hydrogen Ion Concentration
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration: pH = -log[H+]. In electrochemical cells, the pH can influence the concentration of H+ ions, which in turn affects the cell potential. A lower pH indicates a higher concentration of H+ ions, which is crucial for determining the conditions in the anode half-cell.
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06:25Hydronium Ion Concentration Example
Electrochemical Cell Components
An electrochemical cell consists of two half-cells: the anode, where oxidation occurs, and the cathode, where reduction takes place. In the given cell, the anode involves hydrogen gas and protons, while the cathode involves copper ions and solid copper. Understanding the roles of these components and their reactions is essential for analyzing how changes in conditions, such as pH, affect the overall cell potential.
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02:46Electrochemical Cells
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The cell potential of this electrochemical cell depends on the gold concentration in the cathode half-cell. Pt(s) | H2(g, 1.0 atm) | H+(aq, 1.0 M) || Au3+(aq, ? M) | Au(s) What is the concentration of Au3+ in the solution if Ecell is 1.22 V?
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Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. b. 4.85 g Cu
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Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. c. 2.42 g Ag
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