| BACKGROUND
FOR ELECTROCHEMISTRY |
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Oxidation-reduction reactions |
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Oxidation number |
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Half-reaction |
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Oxidation and reduction |
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Review of balancing redox reactions |
| VOLTAIC
CELLS |
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Definitions |
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Electrochemical cell |
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Voltaic
cell, also called a galvanic cell |
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Electrolytic cell |
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Construction of voltaic cells |
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Two half-cells that are electrically connected |
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Definition of half-cell |
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Description
of a simple half-cell |
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The
two half-cells must be connected externally by an external electrical
circuit |
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The
two half cells must be connected internally by a bridge |
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Anodes and cathodes |
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Anode
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Cathode
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Comparison
of the anode and the cathode |
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Cell
reaction |
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Drawing and labeling a voltaic cell |
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Using cell notation for voltaic cells |
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Electromotive force |
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Potential difference |
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Electromotive
force |
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Standard
electrode potential – E° |
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The
voltage produced when one half-cell is connected to the reference half-cell and both are at standard conditions |
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The reference half-cell is a platinum
electrode immersed in 1 M H+ and 1 atm H2 |
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Standard
conditions are 25 °C
and 1 atm |
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The
standard electrode potential of the standard hydrogen electrode (SHE) is defined to be exactly zero |
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Standard
electrode potentials are measured in relation to the SHE |
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Reduction
potentials and oxidation potentials |
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Standard
reduction potentials |
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Determining
the strengths of oxidizing and reducing agents |
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Predicting
the direction of spontaneity from standard electrode potentials |
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Writing
reactions in the direction of spontaneity using the ““Left-Right-Below
Diagonal Rule” |
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Standard cell emf ’s |
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Equation |
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Combining
half-reactions to determine standard cell emf ’s |
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Writing
cell reactions |
| FREE
ENERGY AND ELECTROCHEMISTRY |
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Free energy change and work |
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Electrical
energy and work |
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From
physics |
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From
chemistry |
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Cell
potential and electrical work |
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Faraday’s
constant and charge |
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Calculating free-energy changes
from emf ’s |
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Calculating emf’s from
free-energy changes |
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Calculating the equilibrium
constant from emf ’s |
| CONCENTRATION
AND ELECTROCHEMISTRY |
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Nernst equation |
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Reaction
quotient |
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Relationship
among free-energy change, standard free-energy change, and the reaction
quotient |
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Deriving
the Nernst equation |
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The Nernst equation,
spontaneity, and equilibrium |
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The
relationship between Ecell and reaction progress |
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The
relationship between Ecell, spontaneity, and equilibrium |
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Calculating Ecell
under nonstandard conditions |
| ELECTROLYTIC
CELLS |
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Background
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Electrolysis
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Electrolytic
cell |
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Commercial
importance of electrolysis |
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Electrolysis of various substances |
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Background
for electrolytic cells |
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Electrolysis
of molten salts |
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Aqueous
electrolysis |
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Electroplating
of metals |
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Stoichiometry of electrolysis |
| ELECTROLYTIC
CELLS |
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Background |
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Electrolysis
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Electrolytic
cell |
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Commercial
importance of electrolysis |
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Electrolysis of various substances |
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Background
for electrolytic cells |
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Electrolysis
of molten salts |
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Aqueous
electrolysis |
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Electroplating
of metals |
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Stoichiometry of electrolysis |
| REDOX TITRATIONS |
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Similarities
between acid-base titrations and redox titrations |
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Key
points to redox titrations |
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Redox
titration calculations |
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