Electrochemistry Applications of Redox AP Chemistry Chapter 20 Notes.
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Transcript of Electrochemistry Applications of Redox AP Chemistry Chapter 20 Notes.
![Page 1: Electrochemistry Applications of Redox AP Chemistry Chapter 20 Notes.](https://reader036.fdocuments.in/reader036/viewer/2022081414/55144f53550346284e8b5057/html5/thumbnails/1.jpg)
ElectrochemistryElectrochemistry
Applications of RedoxApplications of Redox
AP Chemistry
Chapter 20 Notes
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ReviewReview
Oxidation reduction reactions involve a Oxidation reduction reactions involve a transfer of electrons.transfer of electrons.
OIL- RIGOIL- RIGOxidation Involves LossOxidation Involves LossReduction Involves GainReduction Involves GainLEO-GER LEO-GER Lose Electrons OxidationLose Electrons OxidationGain Electrons ReductionGain Electrons Reduction
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ApplicationsApplicationsMoving electrons is electric current.Moving electrons is electric current. 8H8H+++MnO+MnO44
--+ 5Fe+ 5Fe+2 +2 +5e+5e-- Mn Mn+2 +2 + 5Fe+ 5Fe+3 +3 +4H+4H22OO
Helps to break the reactions into half rxns.Helps to break the reactions into half rxns.
8H8H+++MnO+MnO44--+5e+5e-- Mn Mn+2 +2 +4H+4H22OO
5Fe5Fe+2+2 5Fe 5Fe+3 +3 + 5e+ 5e-- ) )
In the same mixture it happens without doing In the same mixture it happens without doing useful work, but if separateuseful work, but if separate
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H+
MnO4-
Fe+2
Connected this way the reaction startsConnected this way the reaction startsStops immediately because charge builds Stops immediately because charge builds
up.up.
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H+
MnO4-
Fe+2
Galvanic CellGalvanic Cell
Salt Bridge allows current to flow
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H+
MnO4-
Fe+2
e-
Electricity travels in a complete circuitElectricity travels in a complete circuit Instead of a salt bridgeInstead of a salt bridge
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H+
MnO4-
Fe+2
Porous Disk
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Reducing Agent
Oxidizing Agent
e-
e-
e- e-
e-
e-
Anode Cathode
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Cell PotentialCell Potential
Oxidizing agent pushes the electron.Oxidizing agent pushes the electron.Reducing agent pulls the electron. Reducing agent pulls the electron. The push or pull (“driving force”) is called The push or pull (“driving force”) is called
the cell potential the cell potential EEcellcell
Also called the electromotive force (emf) Also called the electromotive force (emf) Unit is the volt(V) Unit is the volt(V) = 1 joule of work/coulomb of charge= 1 joule of work/coulomb of chargeMeasured with a voltmeterMeasured with a voltmeter
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Zn+2 SO4-
2
1 M HCl
Anode
0.76
1 M ZnSO4
H+
Cl-
H2 in
Cathode
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1 M HCl
H+
Cl-
H2 in
Standard Hydrogen Standard Hydrogen ElectrodeElectrode
This is the reference This is the reference all other oxidations all other oxidations are compared toare compared to
EEº = 0º = 0 º indicates standard º indicates standard
states of 25ºC, 1 atm, states of 25ºC, 1 atm, 1 M solutions.1 M solutions.
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Cell PotentialCell PotentialZn(s) + CuZn(s) + Cu+2 +2 (aq)(aq) Zn Zn+2+2(aq)(aq) + Cu(s) + Cu(s)The total cell potential is the sum of the The total cell potential is the sum of the
potential at each electrode.potential at each electrode.
EEºº cellcell = = EEººZnZn Zn Zn+2+2 + + EEºº CuCu+2+2 CuCu
We can look up reduction potentials in a We can look up reduction potentials in a table.table.
One of the reactions must be reversed, so One of the reactions must be reversed, so change it sign.change it sign.
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Cell PotentialCell Potential
Determine the cell potential for a galvanic Determine the cell potential for a galvanic cell based on the redox reaction.cell based on the redox reaction.
Cu(s) + FeCu(s) + Fe+3+3(aq)(aq) Cu Cu+2+2(aq)(aq) + Fe + Fe+2+2(aq)(aq)
FeFe+3+3(aq)(aq) + e+ e-- Fe Fe+2+2(aq) (aq) EEº = 0.77 Vº = 0.77 V
CuCu+2+2(aq)+2e(aq)+2e-- Cu(s) Cu(s) EEº = 0.34 Vº = 0.34 V
Cu(s) Cu(s) CuCu+2+2(aq)+2e(aq)+2e-- EEº = -0.34 Vº = -0.34 V
2Fe2Fe+3+3(aq)(aq) + 2e+ 2e-- 2Fe 2Fe+2+2(aq) (aq) EEº = 0.77 Vº = 0.77 V
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Line NotationLine Notation
solidsolidAqueousAqueousAqueousAqueoussolidsolidAnode on the leftAnode on the leftCathode on the rightCathode on the rightSingle line different phases.Single line different phases.Double line porous disk or salt bridge.Double line porous disk or salt bridge. If all the substances on one side are If all the substances on one side are
aqueous, a platinum electrode is indicated.aqueous, a platinum electrode is indicated.For the last reactionFor the last reactionCu(s)Cu(s)CuCu+2+2(aq)(aq)FeFe+2+2(aq),Fe(aq),Fe+3+3(aq)(aq)Pt(s)Pt(s)
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Galvanic CellGalvanic Cell
The reaction always runs spontaneously in The reaction always runs spontaneously in the direction that produced a positive cell the direction that produced a positive cell potential.potential.
Four things for a complete description.Four things for a complete description.
1)1) Cell PotentialCell Potential
2)2) Direction of flowDirection of flow
3)3) Designation of anode and cathodeDesignation of anode and cathode
4)4) Nature of all the components- electrodes Nature of all the components- electrodes and ionsand ions
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PracticePractice
Completely describe the galvanic cell Completely describe the galvanic cell based on the following half-reactions under based on the following half-reactions under standard conditions.standard conditions.
MnOMnO44-- + 8 H + 8 H++ +5e +5e-- Mn Mn+2 +2 + 4H+ 4H22OO
EEº=1.51º=1.51FeFe+3+3 +3e +3e-- Fe(s) Fe(s) EEº=0.036Vº=0.036V
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Potential, Work and Potential, Work and GG
emf = potential (V) = work (J) / Charge(C)emf = potential (V) = work (J) / Charge(C)EE = work done by system / charge = work done by system / chargeEE = -w/q = -w/qCharge is measured in coulombs.Charge is measured in coulombs. -w = q-w = qEE Faraday = 96,485 C/mol eFaraday = 96,485 C/mol e--
q = nF = moles of eq = nF = moles of e-- x charge/mole e x charge/mole e--
w = -qw = -qEE = -nF = -nFE E = = G G
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Potential, Work and Potential, Work and GG
Gº = -nFGº = -nFE E ºº if if E E º < 0, then º < 0, then Gº > 0 spontaneousGº > 0 spontaneous if if E E º > 0, then º > 0, then Gº < 0 nonspontaneousGº < 0 nonspontaneous In fact, reverse is spontaneous.In fact, reverse is spontaneous.Calculate Calculate Gº for the following reaction:Gº for the following reaction:CuCu+2+2(aq)+ Fe(s) (aq)+ Fe(s) Cu(s)+ FeCu(s)+ Fe+2+2(aq)(aq)
FeFe+2+2(aq)(aq) + e+ e--Fe(s)Fe(s) EEº = 0.44 Vº = 0.44 V
CuCu+2+2(aq)+2e(aq)+2e-- Cu(s) Cu(s) EEº = 0.34 Vº = 0.34 V
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Cell Potential and Cell Potential and ConcentrationConcentration
Qualitatively - Can predict direction of change Qualitatively - Can predict direction of change
in in EE from LeChâtelier. from LeChâtelier.2Al(s) + 3Mn2Al(s) + 3Mn+2+2(aq) (aq) 2Al 2Al+3+3(aq) + 3Mn(s)(aq) + 3Mn(s)
Predict if Predict if EEcellcell will be greater or less than will be greater or less than EEººcellcell
if [Alif [Al+3+3] = 1.5 M and [Mn] = 1.5 M and [Mn+2+2] = 1.0 M] = 1.0 M if [Alif [Al+3+3] = 1.0 M and [Mn] = 1.0 M and [Mn+2+2] = 1.5M] = 1.5M if [Alif [Al+3+3] = 1.5 M and [Mn] = 1.5 M and [Mn+2+2] = 1.5 M ] = 1.5 M
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The Nernst EquationThe Nernst EquationG = G = Gº +RTln(Q)Gº +RTln(Q) -nF-nFEE = -nF = -nFEEº + RTln(Q)º + RTln(Q)
EE = = EEº - º - RTRTln(Q)ln(Q)
nF nF2Al(s) + 3Mn2Al(s) + 3Mn+2+2(aq) (aq) 2Al 2Al+3+3(aq) + 3Mn(s) (aq) + 3Mn(s)
EEº = 0.48 Vº = 0.48 V Always have to figure out n by balancing.Always have to figure out n by balancing. If concentration can gives voltage, then If concentration can gives voltage, then
from voltage we can tell concentration.from voltage we can tell concentration.
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The Nernst EquationThe Nernst EquationAs reactions proceed concentrations of As reactions proceed concentrations of
products increase and reactants decrease.products increase and reactants decrease.
Reach equilibrium where Q = K and Reach equilibrium where Q = K and EEcellcell
= 0= 0
0 = 0 = EEº - º - RTRTln(K)ln(K)
nFnF
EEº = º = RTRTln(K)ln(K)
nF nF
nFnFEEº º = ln(K)= ln(K)
RTRT
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Batteries are Galvanic CellsBatteries are Galvanic Cells
Car batteries are lead storage batteries.Car batteries are lead storage batteries.Pb +PbOPb +PbO22 +H +H22SOSO44 PbSOPbSO44(s) +H(s) +H22OO
Dry CellDry Cell Zn + NHZn + NH44
++ +MnO +MnO2 2 Zn Zn+2 +2 + NH+ NH3 3 + H+ H22OO
AlkalineAlkaline Zn +MnOZn +MnO2 2 ZnO+ Mn ZnO+ Mn22OO3 3 (in base)(in base)
NiCadNiCad NiONiO22 + Cd + 2H + Cd + 2H22O O Cd(OH) Cd(OH)2 2 +Ni(OH)+Ni(OH)22
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CorrosionCorrosion
Rusting - spontaneous oxidation.Rusting - spontaneous oxidation.Most structural metals have reduction Most structural metals have reduction
potentials that are less positive than Opotentials that are less positive than O22 . .
Fe Fe Fe Fe+2+2 +2e+2e-- EEº= 0.44 Vº= 0.44 V
OO22 + 2H + 2H22O + 4eO + 4e- - 4OH4OH-- EEº= 0.40 Vº= 0.40 V
FeFe+2+2 + O + O2 2 + H+ H22O O FeFe2 2 OO3 3 + H+ H++
Reaction happens in two places.Reaction happens in two places.
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Water
Rust
Iron Dissolves- Fe Fe+2
e-
Salt speeds up process by increasing conductivity
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Preventing CorrosionPreventing Corrosion
Coating to keep out air and water.Coating to keep out air and water.Galvanizing - Putting on a zinc coatGalvanizing - Putting on a zinc coatHas a lower reduction potential, so it is Has a lower reduction potential, so it is
more. easily oxidized.more. easily oxidized.Alloying with metals that form oxide coats.Alloying with metals that form oxide coats.Cathodic Protection - Attaching large Cathodic Protection - Attaching large
pieces of an active metal like magnesium pieces of an active metal like magnesium that get oxidized instead.that get oxidized instead.
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Running a galvanic cell backwards.Running a galvanic cell backwards.Put a voltage bigger than the potential and Put a voltage bigger than the potential and
reverse the direction of the redox reaction.reverse the direction of the redox reaction.Used for electroplating.Used for electroplating.
ElectrolysisElectrolysis
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1.0 M
Zn+2
e- e-
Anode Cathode
1.10
Zn Cu1.0 M
Cu+2
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1.0 M
Zn+2
e- e-
AnodeCathode
A battery >1.10V
Zn Cu1.0 M
Cu+2
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Calculating platingCalculating plating
Have to count charge.Have to count charge.Measure current Measure current II (in amperes) (in amperes)1 amp = 1 coulomb of charge per second1 amp = 1 coulomb of charge per secondq = q = II x t x tq/nF = moles of metalq/nF = moles of metalMass of plated metalMass of plated metalHow long must 5.00 amp current be How long must 5.00 amp current be
applied to produce 15.5 g of Ag from Agapplied to produce 15.5 g of Ag from Ag++
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Other usesOther uses
Electroysis of water.Electroysis of water.Seperating mixtures of ions.Seperating mixtures of ions.More positive reduction potential means More positive reduction potential means
the reaction proceeds forward. the reaction proceeds forward. We want the reverse.We want the reverse.Most negative reduction potential is Most negative reduction potential is
easiest to plate out of solution.easiest to plate out of solution.
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BalancingRedox
Equations
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2. in baseAm3+(aq) + S2O8
2-(aq) ---->
AmO2+(aq) + SO4
2-(aq)
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3. MnO4-(aq) + H2C2O4(aq)
Mn2+(aq) + CO2(g)
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4. Bi(OH)3 + SnO22-
Bi(s) + SnO32-
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ELECTROLYTICCELLS
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Electrolytic Cell
a cell that uses electrical energy to produce a chemical change that would
otherwise NOT occur spontaneously
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Process referred to
as electrolysis
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(+) (-)
M MM+(aq)
X-(aq)
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(+) (-) e-e-
M+(aq)
X-(aq)M M
AnodeM M+ + e-
oxidation
CathodeM+ + e- M reduction
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Ampere a unit of electrical
current equal to one coulomb of charge
per second
1 amp = 1 coulsec
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Coulomba unit of electric
charge equal to the quantity of charge in
about 6 x 1019 electrons
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Faradaya constant
representing the charge on one mole
of electrons
1 F = 96,485 C96,500 C
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3: It is necessary to replate a silver teapot with 15.0 g of silver. If the electrolytic cell runs at 2.00 amps, how long will it take to plate the teapot?
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4: Sodium metal and chlorine gas are prepared industrially in a Down’s Cell from the electrolysis of molten NaCl. What mass of metal and volume of gas can be made per day if the cell operates at 7.0 volts and 4.0 x 104 amps if the cell is 75% efficient?
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5: At what current must a cell be run in order to produce 5.0 kg of aluminum in 8.0 hours if the cell produces solid aluminum from molten aluminum chloride?
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ELECTROCHEMISTRY,FREE ENERGY, & EQUILIBRIUM
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)C(eargch
)J(work)V(emf
q
wE
thus: wmax = - q . Emax
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but: wmax = G
and q = nF
thus if: wmax = - q . Emax
then G = - nFE
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G = G0 + RT ln Q
G = - nFE
- nFE = - nFE0 + RT ln Q
Q lnnF
RTEE 0
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NERNST EQUATION
Q lnnF
RTEE 0
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if: aA + bB cC + dD
Q lnnF
RTEE 0
ba
dc
BA
DCQ
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IF T = 250C = 298.15 K ln Q = 2.303 log Q R = 8.314 J/mol.K F = 96,485 C/mol
Q lnnF
RTEE 0
Q logn
0592.0EE 0
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what if : Q = Keq ?
then: E = 0.0 V
Q lnnF
RTEE 0
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K lnnF
RTE0
K logn
0592.0E0
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6: Calculate the equilibrium constant at 400C for the cell:
Cd(s) Cd2+ (1M) Pb2+ (1M) Pb(s)
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7a: Calculate the standard free energy for the cell:
Cr(s) Cr3+ (1M) Fe2+ (1M) Fe(s)
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7a: Calculate the standard free energy for the cell:
Cr(s) Cr3+ (1M) Fe2+ (1M) Fe(s)
7b: What will be the voltage if [Fe2+] = 0.50M and [Cr3+] = 0.30M at 200C?
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8: Through electrochemical
calculations, determine the Ksp for silver bromide.
AgBr + e- Ag + Br- E0 = 0.10 V
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Review of Redox & Review of Redox & Electrochemical CellsElectrochemical Cells
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ReviewOxidation: loss of e-
[increase in ox #] [reducing agent]Reduction: gain of e-
[decrease in ox #] [oxidizing agent]
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Reduction Potential
The ease with which a chemical species can
be reduced
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Standard ReductionPotential
Appendix MTable 20.1 in text
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1. Which of the following elements listed is the best
reducing agent?CuZnFeAgCr
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2a. Choosing from among the reactants in the given half reactions, identify the strongest and weakest oxidizing agents.
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Anode and CathodeAnode and Cathode OXIDATION OXIDATION occurs at the occurs at the ANODEANODE.. REDREDuction occurs at the uction occurs at the CATCAThode.hode.
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Electrochemical Celldevice in which
chemical energy is spontaneously
changed to electrical energy
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battery
voltaic cell
galvanic cell
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An electrochemical cell consists of ???
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M1 M2
M1+(aq)
X-(aq) X-(aq)
M2+(aq)
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M1 M2
M1+(aq)
X-(aq) X-(aq)
M2+(aq)
AnodeM1 M1
+ + e-
CathodeM2
+ + e- M2
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M1 M2
M1+(aq)
X-(aq) X-(aq)
M2+(aq)
AnodeM1 M1
+ + e-
CathodeM2
+ + e- M2
K+(aq) NO3-(aq)
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e- flow is from source of high
“concentration” to source of low “concentration”
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M1 M2
M1+(aq)
X-(aq) X-(aq)
M2+(aq)
AnodeM1 M1
+ + e-
CathodeM2
+ + e- M2
K+(aq) NO3-(aq)e-
e-
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shorthand notationoxidation reduction
M1 | M1+ || M2
+ | M2 anode cathode
e- flow
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this e- flow can accomplish work
)C(eargch
)J(work)V(emf
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Electrochemical Standard State
Conditions
[ions] = 1 MT = 250C
Pgas = 1 atm
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An electrochemical cell is spontaneous if:
Oxidation-reduction occursEred + Eox > 0
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2b. Which of the oxidizing agents listed is (are) capable of oxidizing Br- to BrO3
- ?
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Line Notation:
ANODE CATHODENi(s)|Ni2+ (aq, 1 M)||Au3+(aq, 1 M)|Au(s) oxidation reduction
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Line Notation:
ANODE CATHODE Al(s) | Al3+(aq, 1 M) || Ni2+(aq, 1 M) | Ni (s)
oxidation reduction