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: Consider the redox reaction: PbO2(s)  +  Ba(s)  +  4H(aq)  →  Pb+2 (aq)  +  Ba +2 (aq) + 2H2O(l)  At standard conditions ε° = 4.36 V (highly spontaneous). Suppose the voltage ε, is measured for the above reaction when the [H+] concentration is [H+] = 10 -7 M instead of [H+] = 1M. How does ε compare to ε° (circle one): ε > ε°        ε < ε°         ε = ε°        Can't be determined

Solution: Consider the redox reaction: PbO2(s)  +  Ba(s)  +  4H+ (aq)  →  Pb+2 (aq)  +  Ba +2 (aq) + 2H2O(l)  At standard conditions ε° = 4.36 V (highly spontaneous). Suppose the voltage ε, is measured for th

Problem

Consider the redox reaction:

PbO2(s)  +  Ba(s)  +  4H(aq)  →  Pb+2 (aq)  +  Ba +2 (aq) + 2H2O(l) 

At standard conditions ε° = 4.36 V (highly spontaneous). Suppose the voltage ε, is measured for the above reaction when the [H+] concentration is [H+] = 10 -7 M instead of [H+] = 1M.

How does ε compare to ε° (circle one):

ε > ε°        ε < ε°         ε = ε°        Can't be determined