Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee 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: Use the standard reduction potentials below to determine which element or ion is the best reducing agent. Pd2+ (aq) + 2 e –       →      Pd (s) E° = + 0.90 V 2 H+ (aq) + 2 e –        →        H2 (g) E° = 0.00 V Mn2+ (aq) + 2 e –       →      Mn (s) E° = – 1.18 V   a) Pd (s)             b) H + (aq)              c) Mn2+ (aq)              d) H2 (g)

Problem

Use the standard reduction potentials below to determine which element or ion is the best reducing agent.

Pd2+ (aq) + 2 e        →      Pd (s) E° = + 0.90 V

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

Mn2+ (aq) + 2 e        →      Mn (s) E° = – 1.18 V

 

a) Pd (s)             b) H + (aq)              c) Mn2+ (aq)              d) H2 (g)