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: Given the measured cell potential, Ecell, is -0.3641 V at 25 °C in the following cell, calculate the H+ concentration Pt (s) | H2(g, 0.769 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 2H+(aq) + 2e- → H2(g)                  E° = 0.00 V Cd2+ (aq) + 2e- → Cd(s)               E° = -0.403 V

Problem

Given the measured cell potential, Ecell, is -0.3641 V at 25 °C in the following cell, calculate the H+ concentration 

Pt (s) | H2(g, 0.769 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) 

The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 

2H+(aq) + 2e- → H2(g)                  E° = 0.00 V 

Cd2+ (aq) + 2e- → Cd(s)               E° = -0.403 V