Domanda del libro di testo
Which metal cation is the best oxidizing agent? a. Pb2+ b. Cr3+ c. Fe2+ d. Sn2+
1359
views
Ch.19 - Electrochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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 62a,b
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. O2(g) + 2 H2O(l) + 4 Ag(s) → 4 OH–(aq) + 4 Ag+(aq) b. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)
Guida verificata passo dopo passo1
Step 1: Identify the half-reactions. The reduction half-reaction is O2(g) + 2 H2O(l) + 4 e- → 4 OH-(aq). The oxidation half-reaction is 4 Ag(s) → 4 Ag+(aq) + 4 e-.
Step 2: Look up the standard reduction potentials for each half-reaction in a table of standard reduction potentials. The standard reduction potential for the reduction of O2 to OH- is +0.40 V. The standard reduction potential for the oxidation of Ag to Ag+ is +0.80 V.
Step 3: Calculate the standard cell potential (Ec°ell) using the formula Ec°ell = E°cathode - E°anode. In this case, the cathode is the reduction half-reaction and the anode is the oxidation half-reaction.
Step 4: If the calculated Ec°ell is positive, the reaction is spontaneous as written. If it is negative, the reaction is non-spontaneous as written.
Step 5: Remember that standard cell potentials are calculated under standard conditions (1 M concentrations, 1 atm pressure, 25°C). If the conditions are different, the actual cell potential may be different from the standard cell potential.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
5mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
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). The overall cell potential for a redox reaction can be calculated by subtracting the reduction potential of the anode from that of the cathode, indicating whether the reaction can occur spontaneously.
Video consigliato:
Percorso guidato
01:27
Standard Cell Potential
Redox Reactions
Redox reactions involve the transfer of electrons between two species, where one is oxidized (loses electrons) and the other is reduced (gains electrons). In these reactions, the oxidation state of the elements changes, and they can be balanced using half-reactions. Understanding the oxidation states and identifying the oxidizing and reducing agents is crucial for analyzing redox processes.
Video consigliato:
Percorso guidato
03:12Identifying 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 cell potential (Ec°ell). If Ec°ell is positive, the reaction is spontaneous as written; if negative, it is non-spontaneous. This concept is rooted in thermodynamics, where spontaneous processes tend to increase the overall entropy of the system.
Video consigliato:
Percorso guidato
04:20Spontaneity of Processes
Pratica correlata
Domanda del libro di testo
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. c. PbO2(s) + 4 H+(aq) + Sn(s) → Pb2+(aq) + 2 H2O(l) + Sn2+(aq)
861
views
Domanda del libro di testo
Determine whether or not each metal dissolves in 1 M HIO3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au b. Cr
1250
views
Domanda del libro di testo
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)
444
views
Domanda del libro di testo
Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. 2 Cu(s) + Mn2+(aq) → 2 Cu+(aq) + Mn(s)
1221
views