Ch.18 - ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: For the following electrochemical cell Cu(s) | Cu2+ (aq, 0.0155M) || Ag+ (aq, 3.50M) | Ag(s)Write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following

Problem

For the following electrochemical cell Cu(s) | Cu2+ (aq, 0.0155M) || Ag+ (aq, 3.50M) | Ag(s)

Write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following values at 25°C using standard potentials as needed.

E cell° = ?V

E cell = ?V


Solution

Use the cell notation to determine the redox reaction and use the Nernst equation to determine the Ecell. Standard Ecell or Eocell will be determine using the standard potential of the cathode and anode

Step 1. Determine the redox reaction

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