Lecture #2 of 18 - UCI Department of Chemistryardo/echem/UCI-CHEM248-2017W_lecture… · IUPAC...

55

Lecture #2 of 18

56

Q: What’s in this set of lectures?

A: Introduction, Review, and B&F Chapter 1, 15 & 4 main concepts:

● Section 1.1: Redox reactions

● Chapter 15: Electrochemical instrumentation

● Section 1.2: Charging interfaces

● Section 1.3: Overview of electrochemical experiments

● Section 1.4: Mass transfer and Semi-empirical treatment of

electrochemical observations

● Chapter 4: Mass transfer

57

Looking forward… our review of Chapter “0”

● Cool applications

● Redox half-reactions

● Balancing electrochemical equations

● History of electrochemistry

● IUPAC terminology and Ecell = Ered – Eox

● Nernst equation and Common reference electrodes

● Standard and Absolute potentials

● Latimer and Pourbaix diagrams

● Calculating Ecell under non-standard state conditions

● Conventions

58A Short History Lesson…

Electrochemistry associated with Luigi Galvani who discovered

“animal electricity,” while trying to Frankenstein frogs legs (1791)

Luigi Galvani(1737–1798)

from Wiki

Physician, Physicist, Philosopher

59Voltaic pileInvented by Alessandro Volta (1800) but the elements of the pile

(galvanic cells) were named after Galvani.

(salt water)

What are the half-reactions?

At the Tempio Voltiano (the Volta Temple)

near Volta's home in Como, Italy.

http://en.wikipedia.org/wiki/Voltaic_pile

Alessandro Volta(1745–1827)

from Wiki

Volta presenting his "Voltaic

Pile" to Napoleon and his

court… and now he is a Count!

http://en.wikipedia.org/wiki/Alessandro_Volta

Physicist

http://en.wikipedia.org/wiki/Voltaic_pile

http://en.wikipedia.org/wiki/Alessandro_Volta

60Galvanic Cells

Physically separating the

half-reactions allows the

electrons to go over a

long distance, from the

anode to the cathode via

a conductor: basis for

conversion of chemical

energy into electricity!

Salt bridge is an ionic conduit to

prevent buildup of charge in both

compartments and also to prevent

bulk mixing of the two solutions

Every non-equilibrium

cell is a galvanic cell (in

one direction, i.e. the

spontaneous direction)

61Electrolysis of waterVolta’s results were shared with

the scientific community and then,

boom, many people demonstrated

electrolysis the same year, and

later, electroplating!

William Cruickshank(17??–1810(1))

Johann Wilhelm Ritter(1776–1810)

Sir Anthony Carlisle(1768–1840)

William Nicholson(1753–1815)

http://en.wikipedia.org/wiki/Johann_Wilhelm_Ritter

Chemist

Chemist Surgeon

Chemist

http://en.wikipedia.org/wiki/Johann_Wilhelm_Ritter

62Daniell (galvanic) Cell (1836)

Half-reactions are

physically separated!

anode

oxidation

cathode

reduction

Zn (s) Zn2+ (aq) + 2e– Cu2+ (aq) + 2e– Cu (s)

NET REACTION: Zn (s) + Cu2+ (aq) Zn2+ (aq) + Cu (s)

John Frederic Daniell(1790–1845)

from Wiki

No more H2 from the

(primary) battery!

Chemist, Meteorologist

63Voltage Produced by Galvanic Cells

The difference in electric

potential between the anode

and the cathode is called:

Cell potential

Cell voltage

emf (electromotive force)

Cell DiagramZn (s) + Cu2+ (aq) Cu (s) + Zn2+ (aq)

[Cu2+] = 1 M and [Zn2+] = 1 M

Zn (s) | Zn2+ (1 M) || Cu2+ (1 M) | Cu (s)

anode cathodesalt bridge

This is horribleIt should be –0.76 V!

64EXAMPLE: What is the standard potential of an electrochemical

cell made of a Cd electrode in a 1.0 M Cd(NO3)2 solution and a

Cr electrode in a 1.0 M Cr(NO3)3 solution?

Cd2+ (aq) + 2e– Cd (s) E0 = -0.40 V

Cr3+ (aq) + 3e– Cr (s) E0 = -0.74 V

Cd2+ will get reduced to Cd

Cr will get oxidized to Cr3+

… thus, it is reducing

2e– + Cd2+ (1 M) Cd (s)

Cr (s) Cr3+ (1 M) + 3e–Anode (oxidation):

Cathode (reduction):

2Cr (s) + 3Cd2+ (1 M) 3Cd (s) + 2Cr3+ (1 M)

x 2

x 3

E0 = Ecathode – Eanodecell0 0

E0 = -0.40 V – (-0.74 V) cell

E0 = +0.34 V (positive = spontaneous)cell

More negative of the two

Which half-reaction is reducing?

Zn Cu

Zn(s) Zn2+(aq) Cu2+(aq) Cu(s)

– –

low impedance to measure current

Zn | Zn2+(aq) || Cu2+(aq) | Cu

IcellJohn Frederic Daniell

(1790–1845)from Wiki

Chemist, Meteorologist

The Daniell Cell (1836)

Zn Cu


– –



Icell

This only works for

less than one second

and then stops due to

Kirchhoff’s current law,

which states that all

current at each location

must sum to zero…

… capacitive charging



Zn Cu

– –

Ai+

Bi–

Icell

Now it

works!

Salt bridge

contains an

inert, redox

inactive salt

solution

(electrolyte)




Zn Cu

– –

Ai+

Bi–


Icell



* Name this cell type

* Identify anode

* Identify cathode

* Name the

electrode signs


Zn Cu

– –

Ai+

Bi–


Icell



* Name this cell type

* Identify anode

* Identify cathode

* Name the

electrode signs

* primary galvanic cell

(A/–) (C/+)


Zn Cu

– –

Ai+

Bi–


Icell




(A/–) (C/+)

This will eventually fully

discharge and reach

equilibrium (ΔG = Ecell = 0)

Then, either direction of

polarization bias results

in electrolytic function

(i.e. charging)!

71Electrochemistry:

conventions… oh, conventions!

Cathode – electrode where catholyte species are reduced

Anode – electrode where anolyte species are oxidized

72Electrochemistry:




Negative/Positive electrode – cathode or anode?… it depends!

For the discharging (galvanic) battery, label the anode and cathode.

http://autoshop101.com/


73Electrochemistry:




Negative/Positive electrode – cathode or anode?… it depends!

For the charging (electrolytic) battery, label the anode and cathode.


e– e–

anodecathode

This is a generator

(AKA power supply)


74Electrochemistry:




… Sheesh!

… Take-home message: For batteries, don’t call electrodes

anodes and cathodes (but convention used by most is for

discharging)


anode

e– e–

cathode

cathodeanode

e– e–


75PROBLEM TIME!

You try!

(a) What is the standard Ecell for agalvanic cell based on zinc and silver?

(b) If we wanted to electrolyticallycharge the cell from part a (beforeany reactions took place), whatpotential would we have to apply?

76PROBLEM TIME!

You try!

(a) What is the standard Ecell for agalvanic cell based on zinc and silver?

(b) If we wanted to electrolyticallycharge the cell from part a (beforeany reactions took place), whatpotential would we have to apply?

(a) Ecell = +0.80 V – (-0.76 V) = 1.56 V

(b) Ebias < –1.56 V

77

• Coulomb (in units of C = A·s) is the unit of charge (96,485 C are in a mole of singly charged species = Faraday constant, F ≈ 96,500 C/mol ≈ 105 C/mol)

• Electricity is the flow of current (A = C/s) and is negative (cathodic) or positive (anodic) depending on the direction and sign of the current-carrying species (e.g. e–, H+)

• (Electrode) (electric) potential (V or E; in units of V = J/C) is written as a reductionThis relates to Gibbs free energy as ΔG = –RT ln K = –nFEcell (electrical work per mole), and…

… partial molar Gibbs free energy is the electrochemical potential ( 𝜇, in units of J/mol)

Chemical potential (𝜇, in units of J/mol)

Galvani/Inner (electric) potential (ϕ, in units of V)

… and in summary, 𝜇 = 𝜇 + 𝑛𝐹ϕAlso, standard state is a solvent, a solid, and a species at unit activity (~1 M solutes, ~1 bar gases)

Also, E = IR (Ohm’s law) when resistance is constant

• Galvanic cells produce power (in units of W = A x V = C/s x J/C = J/s) by spontaneous redox reactions

• Electrolytic cells require a power input to drive redox reactions; thus, the reactions are thermodynamically unfavorable

• Batteries have anodes and cathodes, but these names change depending on if the battery is being discharged (galvanic) or charged (electrolytic), and so the terminology of negative electrode and positive electrode is preferred

International Union of Pure and Applied

Chemistry (IUPAC)

(Sources: B&F, M3LC course textbook,and http://goldbook.iupac.org/)

(Accepted) Nomenclature and Terminology that you know, but may have forgotten

78













Chemistry (IUPAC)


integrate, over timedifferentiate, with respect to time


79













Chemistry (IUPAC)


E0(Cu2+/0) = +0.34 V vs. SHE

E0(Cu0/2+) = –0.34 V vs. SHE

… is incorrect!

You can subtract redox

potentials but do not change the

sign of the potential and then

call it an oxidation potential!


80













Chemistry (IUPAC)


Based on our current sign convention, it is best

to only write reduction potentials; however, if

we lived in an oxidation-potential-centric world,

we could write them all (i.e. everything) as

oxidation potentials; simply put, it is best to

not mix the conventions and so stick with

reduction potentials

E0(Cu2+/0) = +0.34 V vs. SHE

E0(Cu0/2+) = –0.34 V vs. SHE

… is incorrect!

You can subtract redox

potentials but do not change the

sign of the potential and then

call it an oxidation potential!


81







… and in summary, 𝜇 = 𝜇 + 𝑧𝐹ϕAlso, standard state is a solvent, a solid, and a species at unit activity (~1 M solutes, ~1 bar gases)






Chemistry (IUPAC)



82





Chemical potential (𝝁, in units of J/mol)








Chemistry (IUPAC)


Cannot be

measured

independently!


83













Chemistry (IUPAC)



84













Chemistry (IUPAC)



85













Chemistry (IUPAC)

opposites



86International Union of Pure and Applied

Chemistry (IUPAC)













87

Electrochemical potential of species i in phase β is an energy (J/mol),

𝜇𝑖β=

𝜕𝐺

𝜕𝑛𝑖β

𝑇,𝑝,𝑛𝑗≠𝑖

= 𝜇𝑖β+ 𝑧𝑖𝐹𝜙

β, where

G (Gibbs free energy (J))

ni (amount of species i (mol))

𝜇𝑖 = 𝜇𝑖0 + 𝑅𝑇 ln 𝑎𝑖 (chemical potential (J/mol))

zi (valency of species i)

F ≈ 105 (Faraday constant (C/mol)

ϕβ (Galvani/inner electric potential (V))

ai (activity of species i)

For an uncharged species 𝜇𝑖β= 𝜇𝑖

β.

Parsons, Pure & Appl. Chem., 1973, 37, 501

IUPAC Gold (http://goldbook.iupac.org)

A Very Brief (more rigorous) Review of Thermodynamics

FOR YOUR REFERENCE

88Half reactions, at non-unity activity, obey the Nernst equation…

Take ∆𝐺 = ∆𝐺0 + 𝑅𝑇 ln𝑄 and use the relation ∆𝐺 = −𝑛𝐹𝐸,

What is Q?

𝑄 = 𝑝 𝑎𝑝

𝑣𝑝

𝑟 𝑎𝑟𝑣𝑟=

𝑝 γ𝑝𝑐𝑝

𝑐𝑝0

𝑣𝑝

𝑟 γ𝑟𝑐𝑟𝑐𝑟0

𝑣𝑟 , because 𝜇𝑖 = 𝜇𝑖0 + 𝑅𝑇 ln 𝑎𝑖

𝑄 = 𝑝 𝑐𝑝

𝑣𝑝

𝑟 𝑐𝑟𝑣𝑟

, for dilute solutions… which we never have, and where

ap is the activity of product p

ar is the activity of reactant r

vi is the stoichiometric number of i

γi is the activity coefficient of i

ci is the concentration of i

ci0 is the standard state concentration of i



But first… what is Q, again? … the reaction quotient!


𝑣𝑝


𝑝 γ𝑝𝑐𝑝

𝑐𝑝0

𝑣𝑝


𝑣𝑟 , because 𝜇𝑖 = 𝜇𝑖0 + 𝑅𝑇 ln 𝑎𝑖


𝑣𝑝


, for dilute solutions… which we never have, and where









But first… what is Q, again? … the reaction quotient!


𝑣𝑝


𝑝 γ𝑝𝑐𝑝

𝑐𝑝0

𝑣𝑝


𝑣𝑟 , because fundamentally 𝜇𝑖 = 𝜇𝑖0 + 𝑅𝑇 ln 𝑎𝑖


𝑣𝑝


, for dilute solutions… which we never have!








−𝑛𝐹𝐸 = −𝑛𝐹𝐸0 + 𝑅𝑇 ln𝑄

𝐸 = 𝐸0 −𝑅𝑇

𝑛𝐹ln𝑄


Reaction quotient as

product and quotient of

species’ activities

from Wiki

Physicist

Walther Hermann Nernst

(1864–1941)

Nobel Prize (Chemistry, 1920)




𝑛𝐹ln𝑄


𝑛𝐹

log𝑄

log 𝑒


0.4343𝑛𝐹log 𝑄

𝐸 = 𝐸0 −2.3026𝑅𝑇

𝑛𝐹log𝑄





from Wiki

Physicist


(1864–1941)





𝑛𝐹ln𝑄


𝑛𝐹

log𝑄

log 𝑒



𝐸 = 𝐸0 −2.3026𝑅𝑇

𝑛𝐹log𝑄

… and at 298.15 K, 𝐸 = 𝐸0 −0.05916 V

𝑛log 𝑄





from Wiki

Physicist


(1864–1941)





𝑛𝐹ln𝑄


𝑛𝐹

log𝑄

log 𝑒



𝐸 = 𝐸0 −2.3026𝑅𝑇

𝑛𝐹log𝑄

… and at 298.15 K, 𝐸 = 𝐸0 −0.05916 V

𝑛log 𝑄


Remember ~60 mV for log10, but do not forget n and that this is at 25 °C!

from Wiki

Physicist


(1864–1941)





95

standard (SHE)

Rigorously, each needs

to be divided by the

standard-state condition

96

Thus, the potentials for half-cell reactions are actually

full-cell (electric) potential (difference(s)) versus SHE!

standard (SHE)

97

standard (SHE)

* Normal hydrogen electrode (NHE) is an empirical SHE ([H+] = 1; not standard state)* Standard hydrogen electrode (SHE) is a hypothetical, perfect NHE (a = 1; not empirical)* Reversible hydrogen electrode (RHE) is the SHE but the same regardless of pH* And generally, formal potentials (E0’) take into consideration non-idealities and changesin ionic strengths so that the reaction quotient only has concentrations, and not activities

Ramette, J. Chem. Educ., 1987, 64, 885

98

Potential Standard Potential

* Normal hydrogen electrode (NHE) is an empirical SHE ([H+] = 1; not standard state)* Standard hydrogen electrode (SHE) is a hypothetical, perfect NHE (a = 1; not empirical)* Reversible hydrogen electrode (RHE) is the SHE but the same regardless of pH* And generally, formal potentials (E0’) take into consideration non-idealities and changesin ionic strengths so that the reaction quotient only has concentrations, and not activities

standard (SHE)

Ramette, J. Chem. Educ., 1987, 64, 885

99


standard (SHE)

Given E0 = 0, what is

this experimental redox

potential versus?

100

vs. SHE


standard (SHE)

Given E0 = 0, what is

this experimental redox

potential versus?

101

Look up half-reactions and standard reduction potentials in an

Electrochemical Series table (CRC, B&F Appendix C, WWW):

Anode: E0anode = -0.76 V

Cathode: E0cathode = +1.51 V

Note: Although strictly correct, do not use “–E0” as the “E0 for oxidation”

Note: Be careful to choose the correct half-reaction with MnO4–

Zn Zn2+ + 2e–

MnO4– + 8H+ + 5e– Mn2+ + 4H2O

EXAMPLE: Write a balanced chemical equation and

calculate the standard cell potential for the galvanic cell:

Zn(s) | Zn2+ (1 M) || MnO4– (1 M), Mn2+ (1 M), H+ (1 M) | Pt(s)

102CRC Handbook of Chemistry and Physics, 92nd Edition

http://folk.ntnu.no/andersty/2.%20Klasse/KJ1042%20Termodynamikk%20med%20lab/Lab/

Oppgave%205%20-%20Standard%20reduksjonspotensial/Rapportfiler/E0.pdf

* All values versus SHE

MnO4– + 8H+ + 5e–

Mn2+ + 4H2O

Zn Zn2+ + 2e–

http://folk.ntnu.no/andersty/2. Klasse/KJ1042 Termodynamikk med lab/Lab/Oppgave 5 - Standard reduksjonspotensial/Rapportfiler/E0.pdf

103





To get the balanced overall reaction… ?

Zn Zn2+ + 2e–

MnO4– + 8H+ + 5e– Mn2+ + 4H2O






104





To get the balanced overall reaction, multiply the anode

reaction by 5 and add to 2 times the cathode reaction, giving:

E0cell = E0

cathode – E0anode = 1.51 V + 0.76 V = +2.27 V

Zn Zn2+ + 2e–

MnO4– + 8H+ + 5e– Mn2+ + 4H2O

2MnO4– (aq) + 16H+ (aq) + 5Zn (s) 5Zn2+ (aq) + 2Mn2+ (aq) + 8H2O (l)






105

* All values versus SHE

CRC Handbook of Chemistry and Physics, 92nd Edition

http://folk.ntnu.no/andersty/2.%20Klasse/KJ1042%20Termodynamikk%20med%20lab/Lab/

Oppgave%205%20-%20Standard%20reduksjonspotensial/Rapportfiler/E0.pdf

Q: What is electrochemistry? … one more … (remember this?)

* How negative can Eo be?

http://folk.ntnu.no/andersty/2. Klasse/KJ1042 Termodynamikk med lab/Lab/Oppgave 5 - Standard reduksjonspotensial/Rapportfiler/E0.pdf

106

Example: solvated electrons

Q: What is electrochemistry? … one more …

A: Any process involving the motion/transport of charge – carried

by entities other than unsolvated electrons and holes – through

phase(s), or the transfer of charge across interface(s).

Prof. Robert Hamers (Univ. of Wisconsin)

http://hamers.chem.wisc.edu/people

Zhu, …, Hamers, Nature Materials, 2013, 12, 836

diamond


107First description of conductivity using solvated electrons

Cady, J. Phys. Chem., 1897, 1, 707

During the first part of the twentieth century, E. C. Franklin and C. A. Kraus probably did more to elucidate the chemistry of

liquid ammonia solutions than everybody else combined… It is perhaps little known that their work was prompted by the

research and insight of H. P. Cady, carried out while he was an undergraduate! Whilst working on cobalt ammine

complexes, Cady proposed that ammonia in these (and other “double salts”) must function in a manner akin to water in salts

with water of crystallization. He suggested further that liquid ammonia would probably be found to resemble water in its

physical and chemical properties—thus adding a second to our list of ionizing solvents. Cady’s undergraduate work, carried

out without supervision, published in 1897, was perhaps the first physical chemistry study of liquid ammonia solutions.

Zurek, Edwards, & Hoffman, Angew. Chem. Int. Ed., 2009, 48, 8198

108

Example: solvated electrons

Q: What is electrochemistry? … one more …

A: Any process involving the motion/transport of charge – carried

by entities other than unsolvated electrons and holes – through

phase(s), or the transfer of charge across interface(s).

Prof. Robert Hamers (Univ. of Wisconsin)


Zhu, …, Hamers, Nature Materials, 2013, 12, 836

What is this?

diamond


109Absolute potentials can be measured / approximated…

very carefully…

Trasatti, Pure & Appl. Chem., 1986, 58, 955

Prof. Sergio Trasatti

(Università de Milano, Italy)


very carefully…


FOR YOUR REFERENCE


very carefully…

Trasatti, Electroanal. Chem. Interfac. Electrochem., 1974, 52, 313


Born–Haber cycle:

e(Hg)

𝜇𝑒𝐻𝑔

FOR YOUR REFERENCE


very carefully…



Born–Haber cycle:

e(Hg)

𝜇𝑒𝐻𝑔

… but we need an electrode!

FOR YOUR REFERENCE


very carefully…



Born–Haber cycle:

e(Hg)

𝜇𝑒𝐻𝑔


FOR YOUR REFERENCE


very carefully…


Trasatti, Pure & Appl. Chem., 1986, 58, 955… but we need an electrode!

Born–Haber cycle:

e(Hg)

𝜇𝑒𝐻𝑔

FOR YOUR REFERENCE


very carefully…

Farrell and McTigue, Electroanal. Chem. Interfac. Electrochem., 1982, 139, 37



Born–Haber cycle:

e(Hg)

𝜇𝑒𝐻𝑔


Hg

Pt

FOR YOUR REFERENCE

117

A Latimer diagram is a summary of the E0 values for an element; it is useful for visualizing the complete redox series for an element and for determining when disproportionation will occur.

from Wiki

Oxidation Reduction

1,69 V

Two diagrams of empirical standard potentials…

Wendell Mitchell Latimer

(1893–1955)http://academictree.org/chemistry/peopleinfo.php?pid=24644

Chemist

Latimer, The oxidation states of the elements and their potentials in aqueous solution, 1938

118

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

1,69 V



from Wiki



Chemist


119

Disproportionation – spontaneous and simultaneous reduction and oxidation of a molecule

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

1,69 V



from Wiki



Chemist


120

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

(1) Does Mn2+ disproportionate?(2) What is the standard reduction potential of MnO4

– to MnO2?

1,69 V




121

Reduction: Mn2+ Mno Eo = +1.18 V

Oxidation: Mn2+ Mn3+ Eo = +1.51 V

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

(1) Does Mn2+ disproportionate?(2) What is the standard reduction potential of MnO4

– to MnO2?

1,69 V




122

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

(1) Does Mn2+ disproportionate? NO. Eo = Ered – Eox = 1.18 – 1.51 = –0.33 V(2) What is the standard reduction potential of MnO4

– to MnO2?

1,69 V

Reduction: Mn2+ Mno Eo = +1.18 V

Oxidation: Mn2+ Mn3+ Eo = +1.51 V




123

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction


– to MnO2?ΔGo = -nFEo = -3FEo

1,69 V




124

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction



ΔGo = -nFEo1 + -nFEo

2 = -F((1 x 0.56 V) + (2 x 2.26 V)) = -F(5.08 V)

1,69 V




125

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction



ΔGo = -nFEo1 + -nFEo

2 = -F((1 x 0.56 V) + (2 x 2.26 V)) = -F(5.08 V)Set them equal to each other, and thus, 3Eo = 5.08 and Eo = 1.69 V


1,69 V



1,69 V

126

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction



Recall from before…

1,69 V

127

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction



Recall from before… ???

???

1,69 V

128

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction




???

… anyway, why are

these bottom E0

values not on the

Latimer diagram?

1,69 V

129

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction




???

… anyway, why are

these bottom E0

values not on the

Latimer diagram?

… because they

are at basic/alkaline

standard state with

~1 M OH–!

1,69 V

130

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction




???

What would this E0

value be when at

acidic standard

state?

131Two diagrams of empirical standard potentials…


???

𝐸 = 𝐸𝑎𝑐𝑖𝑑0 −

0.05916 V

𝑛log

𝑀𝑛𝑂21 𝐻2𝑂

2

𝑀𝑛𝑂42− 1

𝐻+ 4= 𝐸𝑎𝑐𝑖𝑑

0 −0.05916 V

2log

1 1

1 1 10−14 4= 𝐸𝑎𝑐𝑖𝑑

0 − 0.02958 V 56

What would this E0

value be when at

acidic standard

state?

1,69 V

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

???

FOR YOUR REFERENCE



???


0.05916 V

𝑛log


2

𝑀𝑛𝑂42− 1


0 −0.05916 V

2log

1 1

1 1 10−14 4= 𝐸𝑎𝑐𝑖𝑑

0 − 0.02958 V 56

What would this E0

value be when at

acidic standard

state?

1,69 V

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

???

FOR YOUR REFERENCE



???

1,69 V

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction

???


0.05916 V

𝑛log


2

𝑀𝑛𝑂42− 1


0 −0.05916 V

2log

1 1

1 1 10−14 4= 𝐸𝑎𝑐𝑖𝑑

0 − 0.02958 V 56

𝐸 = 𝐸𝑎𝑐𝑖𝑑0 − 1.65648 V = 0.60 V

What would this E0

value be when at

acidic standard

state?

FOR YOUR REFERENCE

1,69 V

135

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction



???

???

𝐸 = 𝐸𝑎𝑐𝑖𝑑0 − 1.65648 V = 0.60 V

𝐸𝑆𝐻𝐸0 = 2,25648 V

SWEET!


0.05916 V

𝑛log


2

𝑀𝑛𝑂42− 1


0 −0.05916 V

2log

1 1

1 1 10−14 4= 𝐸𝑎𝑐𝑖𝑑

0 − 0.02958 V 56

What would this E0

value be when at

acidic standard

state?

FOR YOUR REFERENCE

1,69 V

136

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation Reduction



???

???

𝐸 = 𝐸𝑎𝑐𝑖𝑑0 − 1.65648 V = 0.60 V

𝐸𝑆𝐻𝐸0 = 2,25648 V

SWEET!


0.05916 V

𝑛log


2

𝑀𝑛𝑂42− 1


0 −0.05916 V

2log

1 1

1 1 10−14 4= 𝐸𝑎𝑐𝑖𝑑

0 − 0.02958 V 56

… but then why did the

CRC not list this? …

What would this E0

value be when at

acidic standard

state?

137

A Pourbaix diagram is a map of the predominant equilibrium species of an aqueous electrochemical system; it is useful for identifying which materials/species are present/stable

from Wiki

Marcel Pourbaix

(1904–1998)http://corrosion-doctors.org/Biographies/PourbaixBio.htm

… Second one (not truly standard potentials)…

Pourbaix, Atlas of electrochemical equilibria in aqueous solutions, 1974

Chemist



138


from Wiki

Marcel Pourbaix



Chemist

1,69 V

from Wiki

7+ 6+ 4+ 3+ 2+ 0

Oxidation

???




… because in acid, the reaction does

not occur!

139

from Wiki

RHE

E(O2,H+/H2O)

Marcel Pourbaix



Anyway, … standard state is here

Chemist



Why don’t I like this? … Even though EVERYONE does it this way

Lecture #2 of 18 - UCI Department of Chemistryardo/echem/UCI-CHEM248-2017W_lecture… · IUPAC...

Documents

Transcript of Lecture #2 of 18 - UCI Department of Chemistryardo/echem/UCI-CHEM248-2017W_lecture… · IUPAC...