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21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
2 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Electrical PotentialElectrical Potential
Electrical Potential
What causes the electrical potential of an
electrochemical cell?
• The electrical potential of a voltaic cell is a measure of the cell’s ability
to produce an electric current.
• Electrical potential is usually measured in volts (V).
33
Electrons are transferred from Al to Cu2+, but there is no useful electric current. Energy
released as HEAT.
Electrochemical ReactionsElectrochemical Reactions
44If Al and Cu are separated work is done by the electrons. Voltmeter is
used to measure the energy.
What determines
the measured
value?
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
7 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Electrical PotentialElectrical Potential
The potential of an isolated half-cell cannot be measured.
• You cannot measure the electrical potential of a zinc half-cell or of a copper half-cell separately.
• When these two half-cells are connected to form a voltaic cell,
however, the difference in potential can be measured.
88
CELL POTENTIAL, ECELL POTENTIAL, E
• For Zn/Cu cell, this is indicated by a voltage of 1.10 V at 25 ˚C and when
[Zn2+] and [Cu2+] = 1.0 M.
Zn and Zn2+,anode
Cu and Cu2+,cathode
Zn
Zn2+ ions
Cu
Cu2+ ions
wire
saltbridge
electrons
Zn
Zn2+ ions
Cu
Cu2+ ions
wire
saltbridge
electrons1.10 V1.10 V
1.0 M1.0 M 1.0 M1.0 M
99CELL POTENTIAL, ECELL POTENTIAL, E
STANDARD CELL POTENTIAL, Eo
is when [Zn2+] and [Cu2+] = 1.0 M.
For Zn/Cu cell, potential is +1.10 V at 25 ˚C
a quantitative measure of the tendency of reactants to proceed to products when all are
in their standard states at 25 ˚C.
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
10 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Electrical PotentialElectrical Potential
The standard hydrogen electrode is used with other electrodes so the
reduction potentials of the other cells can be measured.
• The standard reduction potential of the hydrogen electrode has been assigned a value of 0.00 V.
1111
CELL POTENTIALS, ECELL POTENTIALS, Eoo
Can’t measure 1/2 reaction Eo directly. Therefore, measure it
relative to a STANDARD HYDROGEN CELL..
2 H+(aq, 1 M) + 2e- <----> H2(g, 1 atm)2 H+(aq, 1 M) + 2e- <----> H2(g, 1 atm)
Eo = 0.0 VSHE
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
13 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Electrical PotentialElectrical Potential
The difference between the reduction potentials of the two half-cells is called
the cell potential.
cell potential = – reduction potential of half-cell in which reduction occurs
reduction potential of half-cell in which
oxidation occurs
or Ecell = Ered – Eoxid
–
1414
Zn/Zn2+ half-cell hooked to a SHE.Eo for the cell = +0.76 V
Zn/Zn2+ half-cell hooked to a SHE.Eo for the cell = +0.76 V
Volts
ZnH2
Salt Bridge
Zn2+ H+
Zn Zn2+ + 2e- OXIDATION ANODE
2 H+ + 2e- H2REDUCTIONCATHODE
- +
Volts
ZnH2
Salt Bridge
Zn2+ H+
Zn Zn2+ + 2e- OXIDATION ANODE
2 H+ + 2e- H2REDUCTIONCATHODE
- +
Negative Negative electrodeelectrode
Supplier Supplier of of
electronselectrons
Acceptor Acceptor of of
electronselectrons
Positive Positive electrodeelectrode
2 H2 H++ + 2e- --> H + 2e- --> H22
ReductionReductionCathodeCathode
Zn --> ZnZn --> Zn2+2+ + 2e- + 2e- OxidationOxidation
AnodeAnode
1616Volts
ZnH2
Salt Bridge
Zn2+ H+
Zn Zn2+ + 2e- OXIDATION ANODE
2 H+ + 2e- H2REDUCTIONCATHODE
- +
Volts
ZnH2
Salt Bridge
Zn2+ H+
Zn Zn2+ + 2e- OXIDATION ANODE
2 H+ + 2e- H2REDUCTIONCATHODE
- +
Zn(s) + 2H+(aq) --> Zn2+ + H2(g) Eo =+0.76 V
Therefore, oxidation potential
Eo for Zn ---> Zn2+ (aq) + 2e- is +0.76 V
Overall: reduction of H+
by Zn metal.
1717
Volts
CuH2
Salt Bridge
Cu2+ H+
Cu2+ + 2e- Cu REDUCTION CATHODE
H2 2 H+ + 2e-OXIDATION ANODE
-+
Volts
CuH2
Salt Bridge
Cu2+ H+
Cu2+ + 2e- Cu REDUCTION CATHODE
H2 2 H+ + 2e-OXIDATION ANODE
-+
Cu/CuCu/Cu2+2+ and H and H22/H/H++ Cell Cell
EEoo = +0.34 V = +0.34 V
Acceptor Acceptor of of
electronselectrons
Supplier Supplier of of
electronselectrons
CuCu2+2+ + 2e- --> Cu + 2e- --> CuReductionReductionCathodeCathode
HH22 --> 2 H --> 2 H++ + 2e- + 2e-
OxidationOxidationAnodeAnode
PositivePositive NegativeNegative
1818
Cu/CuCu/Cu2+2+ and H and H22/H/H++ Cell Cell
Cu2+ (aq) + H2(g) ---> Cu(s) + 2 H+(aq)
Measured Eo = +0.34 VTherefore, reduction potential
Eo for Cu2+ + 2e- ---> Cu is +0.34 V
Volts
CuH2
Salt Bridge
Cu2+ H+
Cu2+ + 2e- Cu REDUCTION CATHODE
H2 2 H+ + 2e-OXIDATION ANODE
-+
Volts
CuH2
Salt Bridge
Cu2+ H+
Cu2+ + 2e- Cu REDUCTION CATHODE
H2 2 H+ + 2e-OXIDATION ANODE
-+
Overall reaction is reduction of Cu2+ by H2 gas.
1919
Calculating Cell VoltageCalculating Cell Voltage
• Balanced half-reactions can be added together to get overall, balanced equation.
Zn(s) ---> ZnZn(s) ---> Zn2+2+(aq) + 2e-(aq) + 2e-CuCu2+2+(aq) + 2e- ---> Cu(s)(aq) + 2e- ---> Cu(s)----------------------------------------------------------------------------------------CuCu2+2+(aq) + Zn(s) ---> Zn(aq) + Zn(s) ---> Zn2+2+(aq) + Cu(s)(aq) + Cu(s)
Zn(s) ---> ZnZn(s) ---> Zn2+2+(aq) + 2e-(aq) + 2e-CuCu2+2+(aq) + 2e- ---> Cu(s)(aq) + 2e- ---> Cu(s)----------------------------------------------------------------------------------------CuCu2+2+(aq) + Zn(s) ---> Zn(aq) + Zn(s) ---> Zn2+2+(aq) + Cu(s)(aq) + Cu(s)
If we know Eo for each half-reaction, we could get Eo for net reaction..
2020
Zn/Cu Electrochemical CellZn/Cu Electrochemical Cell
Zn(s) ---> ZnZn(s) ---> Zn2+2+(aq) + 2e-(aq) + 2e- EEoo = +0.76 V = +0.76 VCuCu2+2+(aq) + 2e- ---> Cu(s)(aq) + 2e- ---> Cu(s) EEoo = +0.34 V = +0.34 V------------------------------------------------------------------------------------------------------------------------------CuCu2+2+(aq) + Zn(s) ---> Zn(aq) + Zn(s) ---> Zn2+2+(aq) + Cu(s) (aq) + Cu(s)
Eo (calc’d) = +1.10 V
Cathode, positive, sink for electrons
Anode, negative, source of electrons
Zn
Zn2+ ions
Cu
Cu2+ ions
wire
saltbridge
electrons
Zn
Zn2+ ions
Cu
Cu2+ ions
wire
saltbridge
electrons ++
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
21 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Electrical PotentialElectrical Potential
The tendency of a given half-reaction to occur as a reduction is called the reduction potential.
• The half-cell in which reduction occurs has a greater reduction potential than the half-cell in which oxidation occurs.
2222
Using Standard Potentials, EUsing Standard Potentials, Eoo
Table 20.1Table 20.1
• Which is the best oxidizing agent (reduced):
O2, H2O2, or Cl2? _________________
• Which is the best reducing agent (oxidized):
Hg, Al, or Sn? ____________________
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
23 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Electrical PotentialElectrical Potential
The standard cell potential (E0cell) is the
measured cell potential when the ion concentrations in the half-cells are 1M,
any gases are at a pressure of 101 kPa, and the temperature is 25°C.
E0cell = E0
red – E0oxid
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
24 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Calculating Standard Calculating Standard Cell PotentialsCell Potentials
Calculating Standard Cell Potentials
How can you determine if a redox reaction is spontaneous?
Positive Cell Potentials
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
25 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Calculating Standard Calculating Standard Cell PotentialsCell Potentials
If the cell potential for a given redox reaction is positive, then the reaction is spontaneous as
written.
If the cell potential is negative, then the reaction is
non-spontaneous.
2626
Uses of EUses of Eoo Values ValuesUses of EUses of Eoo Values Values
• Organize half-reactions by relative ability to act as oxidizing agents (reduced)
• Table 20.1Table 20.1• Use this to predict
cell potentials and direction of redox reactions.
Zn
Zn2+ ions
Cu
Cu2+ ions
wire
saltbridge
electrons
Zn
Zn2+ ions
Cu
Cu2+ ions
wire
saltbridge
electrons
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
29 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Oxidation: Al(s) → Al3+(aq) + 3e– (at anode)
Reduction: Fe3+(aq) + 3e– → Fe(s) (at cathode)
Al(s) + Fe3+(aq) → Al3+(aq) + Fe(s)
Determine the cell reaction for a voltaic cell composed of the following half-cells.
Fe3+(aq) + 3e– → Fe(s) E0cell = –0.036 V
Al3+(aq) + 3e– → Al(s) E0cell = –1.66 V
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
30 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Show that the following redox reaction between zinc metal and silver ions is
spontaneous.
Sample Problem 21.1Sample Problem 21.1
Determining Reaction Spontaneity
Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s)
If E0cell is positive, the reaction is spontaneous.
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
31 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
• First identify the half-reactions.
Sample Problem 21.1Sample Problem 21.1
Oxidation: Zn(s) → Zn2+(aq) + 2e–
Reduction: Ag+(aq) + e– → Ag(s)
• Write both half-cells as reductions with their standard reduction potentials.
Zn2+(aq) + 2e– → Zn(s) E0Zn
2+ = –0.76 V
Ag+(aq) + e– → Ag(s) E0Ag
+ = +0.80 V
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
32 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
• Calculate the standard cell potential.
Sample Problem 21.1Sample Problem 21.1
E0cell = E0
red – E0oxid = E0
Ag+ – E0
Zn2+
= +0.80 V – (–0.76 V) = +1.56 V
E0cell > 0, so the reaction is spontaneous.
3333More About More About Calculating Cell VoltageCalculating Cell Voltage
Assume I- ion can reduce water.
2 H2O + 2e- ---> H2 + 2 OH- Cathode: Red 2 I- ---> I2 + 2e- Anode: Ox-------------------------------------------------2 I- + 2 H2O --> I2 + 2 OH- + H2
2 H2O + 2e- ---> H2 + 2 OH- Cathode: Red 2 I- ---> I2 + 2e- Anode: Ox-------------------------------------------------2 I- + 2 H2O --> I2 + 2 OH- + H2
Assuming reaction occurs as written,
E˚net = E˚cathode - E˚anode or = E˚red + E˚ox
= (-0.828 V) - (+0.535 V) = -1.363 V
Minus E˚ means rxn. occurs in opposite direction
3434
Using Standard Potentials, EUsing Standard Potentials, Eoo
Table 20.1Table 20.1
• In which direction do the following
reactions go?
Cu(s) + 2 Ag+(aq) ---> Cu2+(aq) + 2 Ag(s)
What is Eonet for the overall reaction?
3535Standard Redox Standard Redox Potentials, EPotentials, Eoo
E˚net = “distance” from “top” half-reaction
(cathode) to “bottom” half-reaction (anode)
E˚net = E˚cathode - E˚anode
EEoonetnet for Cu/Ag+ reaction = +0.46 V for Cu/Ag+ reaction = +0.46 V
3636
Volts
Cd Salt Bridge
Cd2+
Fe
Fe2+
Volts
Cd Salt Bridge
Cd2+
Fe
Fe2+
Cd --> Cd2+ + 2e-or
Cd2+ + 2e- --> Cd
Fe --> Fe2+ + 2e-or
Fe2+ + 2e- --> Fe
Eo for a Voltaic Cell
All ingredients are present. Which way does reaction proceed??
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
37 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
In a voltaic cell in which one half-reaction is Fe3+ + 3e– → Fe, which of the following
would occur as oxidation?
A.2H+ + 2e– → H2
B.Al3+ + 3e– → Al
C.Br2 + 2e– → 2Br–
D.Fe3+ + e– → Fe2+
B.
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
38 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Key ConceptsKey Concepts
The electrical potential of a cell results from a competition for electrons between two half-cells.
You can determine the standard reduction potential of a half-cell by using a standard hydrogen electrode and the equation for standard cell potential.
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
39 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Key Concepts & Key Concepts & Key Equation Key Equation
If the cell potential for a given redox reaction is positive, then the reaction is spontaneous as written. If the cell potential is negative, then the reaction is nonspontaneous.
E0cell = E0
red – E0oxid
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
40 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Glossary TermsGlossary Terms
• electrical potential: the ability of a voltaic cell to produce an electric current
• reduction potential: a measure of the tendency of a given half-reaction to occur as a reduction (gain of electrons) in an electrochemical cell
• cell potential: the difference between the reduction potentials of two half-cells
21.2 Half-Cells and Cell Potentials >21.2 Half-Cells and Cell Potentials >
41 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.
Glossary TermsGlossary Terms
• standard cell potential (E0cell): the measured
cell potential when the ion concentrations in the half-cells are 1.00M at 1 atm of pressure and 25°C
• standard hydrogen electrode: an arbitrary reference electrode (half-cell) used with another electrode (half-cell) to measure the standard reduction potential of that cell; the standard reduction potential of the hydrogen electrode is assigned a value of 0.00 V