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: Consider the following standard reduction potentials in acid solution:                                                             E°(V) Al3+ + 3e- → Al(s)                                - 1.66 AgBr(s) + e- → Ag(s) + Br -                   + 0.07 Sn4+ + 2e- → Sn2+                              + 0.14 Fe3+ + e- → Fe2+                                 + 0.77 The strongest oxidizing agent among those shown above is  A) Fe3+. B) Fe2+. C) Br -. D) Al3+. E) Al.

Problem

Consider the following standard reduction potentials in acid solution:

                                                            E°(V)
Al3+ + 3e- → Al(s)                                - 1.66
AgBr(s) + e- → Ag(s) + Br -                   + 0.07
Sn4+ + 2e- → Sn2+                              + 0.14
Fe3+ + e- → Fe2+                                 + 0.77

The strongest oxidizing agent among those shown above is 

A) Fe3+.

B) Fe2+.

C) Br -.

D) Al3+.

E) Al.