Domanda del libro di testo
Determine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Ag
Ch.20 - Electrochemistry
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
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Capitolo 20, Problema 65b,c
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq) c. Cl2(g) + 2 F–(aq) → F2(g) + 2 Cl–(aq)
Guida verificata passo dopo passo1
Identify the half-reactions involved in the redox process. For the given reaction, the half-reactions are: \( \text{MnO}_2 + 4\text{H}^+ + 2e^- \rightarrow \text{Mn}^{2+} + 2\text{H}_2\text{O} \) and \( \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \).
Look up the standard reduction potentials (\( E^\circ \)) for each half-reaction from a standard reduction potential table. The reduction potential for \( \text{MnO}_2 + 4\text{H}^+ + 2e^- \rightarrow \text{Mn}^{2+} + 2\text{H}_2\text{O} \) and the oxidation potential for \( \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \) are needed.
Calculate the standard cell potential (\( E^\circ_{\text{cell}} \)) using the formula: \( E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \). Here, the cathode is the reduction half-reaction and the anode is the oxidation half-reaction.
Determine the spontaneity of the reaction. If \( E^\circ_{\text{cell}} > 0 \), the reaction is spontaneous as written. If \( E^\circ_{\text{cell}} < 0 \), the reaction is non-spontaneous as written.
Summarize the findings: State the calculated \( E^\circ_{\text{cell}} \) and whether the reaction is spontaneous or not based on the sign of \( E^\circ_{\text{cell}} \).
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Standard Electrode Potential (Ec°ell)
The standard electrode potential, Ec°ell, is a measure of the tendency of a chemical species to be reduced, expressed in volts. It is determined under standard conditions (1 M concentration, 1 atm pressure, and 25°C). A positive Ec°ell indicates a spontaneous reaction, while a negative value suggests non-spontaneity. The overall cell potential is calculated by subtracting the reduction potential of the anode from that of the cathode.
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01:27
Standard Cell Potential
Balancing Redox Reactions
Balancing redox reactions involves ensuring that both mass and charge are conserved in the reaction. This is achieved by identifying the oxidation and reduction half-reactions, balancing the atoms involved, and adjusting the electrons transferred. The balanced equation allows for accurate calculations of the standard electrode potentials and helps in determining the spontaneity of the reaction.
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01:04Balancing Basic Redox Reactions
Spontaneity of Reactions
A reaction is considered spontaneous if it occurs without external intervention, which can be determined by the sign of the standard cell potential (Ec°ell). If Ec°ell is positive, the reaction is spontaneous as written; if negative, it is non-spontaneous. This concept is crucial in electrochemistry, as it helps predict the feasibility of redox reactions and their practical applications in batteries and electrolysis.
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04:20Spontaneity of Processes
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