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) | Cu 2+ (aq, 0.0155M) || Ag+ (aq, 3.50M) | Ag(s)Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K.X(s) + Y4+(a

Problem

For the following electrochemical cell Cu(s) | Cu 2+ (aq, 0.0155M) || Ag+ (aq, 3.50M) | Ag(s)

Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K.

X(s) + Y4+(aq) ⇌ X4+(aq) + Y(s) K = 1.65 x 10 3

E° = ?V

Solution

Use the Nernst (Keq-Eocell) equation to determine Eocell of the reaction

Step 1. Determine the values and the working equation

View the complete written solution...