2. What is
electrochemistry?
ï Electrochemistry is the study of
chemical reactions which take place at
the interface of an electrode usually a
solid, metal or semiconductor and an
ionic conductor , the electrolyte.
ï Electrochemistry deals with the
interaction between electrical energy
and chemical change.
3. History of electrochemistry
ï English chemist john Daniel and physicist
Michael faraday both credited as founders
of electrochemistry today.
ï The first germen physicist Otto von
Guericke created the electric
generater,which produced static electricity
by applying friction in the machine.
ï The English scientist William Gilbert spent
17 years experimenting with magnetism
and to a lesser extent electricity.
john
Daniel
Michael
faraday
4. ï The french chemist charles francois de cisternry du fay
had discovered two types of static electricity.
ï William Nicholson and Johann Wilhelm Ritter
succeeded in decomposing water into hydrogen and
oxygen by electrolysis.
ï Ritter discovered the process of electroplating.
ï William Hyde Wollaston made improvements to the
galvanic cells.
ï Orstedâs discovery of the magnetic effect of electrical
currents and further work on electromagnetism to
others.
5. ï Michael Faraday's experiments led him to state his two
laws of electrochemistry and john Daniel invented
primary cells.
ï Paul Heroult and Charles M.Hall developed an
efficient method to obtain aluminum using
electrolysis of molten alumina.
ï Nernst developed the theory of the electromotive force
and his equation known as Nernst equation, which
related the voltages of a cell to its properties.
ï Quantum electrochemistry was developed by Revaz
dogonadeze and his pupils.
6. Oxidation-Reduction
ï The term redox stands for reduction-oxidation
ï It refers to electrochemical processes involving
electron transfer to or from a molecule or iron
changing its states.
ï The atom or molecule which loses electrons is known
as the reducing agent.
ï The substance which accepts the electrons is called the
oxidizing agent.
10. Standard electrode potential
ïTo allow prediction of the cell potential,
tabulations of standard electrode potential are available.
ïTabulations are referenced to the standard hydrogen
electrode.
ïThe standard hydrogen electrode undergoes the reaction
ï
2 H+
(aq) + 2 eâ
â H2
11. ïStandard electrode potentials are usually tabulated
as reduction potentials.
ïThe reactions are reversible and the role of particular
electrode in a cell depends on the relative oxi./red.
Potential of both electrodes.
ïThe cell potential is then calculated as the sum of
reduction potential for cathode and the oxidation
potential for anode.
ïFor example, the standard electrode potential for a
copper electrode is:
Cell diagram
Pt(s) | H2 (1 atm) | H+
(1 M) || Cu2+
(1 M) |
Cu(s)
E°cell = E°red (cathode) â E°red (anode)
12. Gibbs free energy and cell
potential
ïThough cell potential Cell and get electricity n faraday
in the cell:
For standard cell, this equation can we written
ïThough produce of electric energy converted into
electric work,
= -nFEcell
G
0
= -RTlnK=-nFE0
cell
Wmax= Welectrical= -nFEcell
13. Nernst equation
E(M
n+
|M)=E0
(M
n+
|M)- ln
But solid M concentrate constant
E(M
n+
|M)=E0
(M
n+
|M)- ln
Example of Daniel cell
For cathode : E(Cu
2+
|Cu)=E0
(Cu
2+
|Cu)- ln
For anode : E(Zn
2+
|Zn)=E0
(Zn
2+
|Zn)- ln
Cell Potential : Ecell= : E(Cu
2+
|Cu) - E(Zn
2+
|Zn)
= E0
(Cu
2+
|Cu)- ln - E0
(Zn
2+
|Zn)- ln
= Ecell=E0
cell- ln
14. ï Electrical resistivity
ïIt is an intrinsic property that quantities how strongly a
given material opposes the flow of electrical current.
ïMany resistors and conductors have a uniform cross
section with a uniform flow of electric current and made
of one material
ïThe electrical resistivity defined
15. ï Electrical conductivity
ïThe reciprocal of electrical resistivity, and measures a
materialâs ability to conduct an electric current.
ïIt is commonly represented by Ï
ïConductivity is defined as
Conductivity SI units of Siemens per meter.
16. Molar conductivity
ïMolar conductivity is defined as the conductivity of an
electrolyte solution divided by the molar
concentration of the electrolyte, and so measures the
efficiency with which a given electrolyte conducts
electricity in solution.
ïFrom definition, the molar conductivity
17. âą Two cases should be distinguished:
ïStrong eletrolyte and weak electrolyte
ï For strong electrolyte
ïSalts, strong acids and strong bases, the molar
conductivity depends only weakly on concentration.
18. ï For weak electrolyte
ïThe molar conductivity strongly depends on
concentration.
ïThe more dilute a solution, the greater its molar
conductivity, due to increased ionic dissociation.
ïFor weak electrolyte obeys Oswald's dilulation law.
19. Kohlrauschâs law of independent
migration of ions
ïHigh accuracy in dilute solutions, molar conductivity
is composed of individual contributions of ions.
ïLimiting conductivity of anions and cations are
additive, the conductivity of a solution of a salt is equal
to the sum of conductivity contributions from the
cation and anion
Î0
m=v+ Î0
+ +v- Î0
-
20. Battery
ïMany types of battery have been commercialized and
represent an important practical application of
electrochemistry.
ïEarly wet cells powered the first telegraph and
telephone systems, and were the source of current for
electroplating.
ïThe zinc-manganese dioxide dry cell was the first
portable, non-spill able battery type that made
flashlights and other portable devices practical.
21. ïThe mercury battery using zinc and mercuric oxude
provided higher levels of power and capacity than the
original dry cell for early electronic devices.
ïLead-acid battery was secondary battery.
ïThe electrochemical reaction that produced current
was reversible, allowing electrical energy and chemical
energy to be interchanged as needed.
ïLead-acid cells continue to be widely used in
automobiles.
22. ïThe lithium battery, which does not use water in the
electrolyte, provides improved performance over other
types.
ïRechargeable lithium ion battery is an essential part of
many mobile devices.
23. Corrosion
ïCorrosion is the term applied to steel rust caused by an
electrochemical process.
ïCorrosion of iron in the form of reddish rust, black
tarnish on silver, red or green may be appear on copper
and its alloys, such as brass.
24. Prevention of corrosion
ï Coating
ïMetals can be coated with paint or other less
conductive metals.
ïThis prevents the metal surface from being exposed to
electrolytes.
ïScratches exposing the metal substrate will result in
corrosion.
25. âą Sacrificial anodes
ïThe method commonly used to protect a structural
metal is to attach a metal which is more anodic than
the metal to be protected.
ïThis forces the structural metal to be catholic thus
spared corrosion. it is called sacrificial.
ïZinc bars are attached to various locations on steel
ship hulls to render the ship hull catholic.
ïOther metal used magnesium.
26. Electrolysis
ïThe spontaneous redox
reactions of a conventional
battery produce electricity
through the different chemical
potentials of the cathode and
anode in the electrolyte.
ïElectrolysis requires an
external source of electrical
energy to include a chemical
reaction , and this process
takes place in a compartment
called an electrolytic cell.
27. Electrolysis of molten sodium
chlorineïWhen molten, the salt sodium chloride can be
electrolyzed to yield metallic sodium and gaseous
chlorine.
ïThis process takes place in a special cell named
Downâs cell.
ïThis process can yield large amounts of metallic
sodium and gaseous chlorine, and widely used on
mineral dressing and metallurgy industries.
Reactions that take place at Down's cell are the following
Anode (oxidation): 2 Clâ
â Cl2(g) + 2 eâ
Cathode (reduction): 2 Na+
(l) + 2 eâ
â 2 Na(l)
Overall reaction: 2 Na+
+ 2 Clâ
(l) â 2 Na(l) + Cl2(g)
28. Quantitative electrolysis and
Faradayâs law
ïQuantitative aspects of electrolysis were originally
developed by Michel faraday .
ïFaraday is also credited to have coined the terms
electrolyte.
ïElectrolysis among many others while studying
analysis of electrochemical reactions.
ïFaraday advocate of the law of conservation of energy.
29. First law
ï The mass of products yielded on the electrodes was
proportional to the the value of current supplied to the cell,
the length of time the current existed, and the molar mass
of the substance analyzed.
ï The amount of substance deposited on each electrode of an
electrolytic cell is directly proportional to the quantity of
electricity passed through the cell.
m=
30. Second law
ïThe amounts of bodies which are equivalent to each
other in the ordinary chemical action have equal
quantities of of electricity naturally associated with
them.
ïThe quantities of different elements deposited by a
given amount of electricity are in the ratio of the
chemical equivalent weights
31. Applied aspects of
electrochemistry
ïIndustrial electrolytic processes
ïElectrochemical Reactors
ïBatteries
ïFuel cells
ïSome Electrochemical Devices
ïElectrochemical Methods of Analysis
32. Branch of electrochemistry
ï Photo electrochemistry
ïIt is subfield of study within physical chemistry.
ïThe interest in this domain is high in the context of
development of renewable energy conversion and
storage technology.
ïThe effects of luminous radiation on the properties of
electrodes and on electrochemical reactions are the
subject of photo electrochemistry
33. ï Semiconductorâs electrochemistry
ïSemiconductor material has a band gap and generates a
pair of electron and hole per absorbed photon if the
energy of the photon is higher than the band gap of the
semiconductor.
ïThis property of semiconductor materials has been
successfully used to converted solar energy into electrical
energy by photovoltaic devices.
ï Semiconductor-electrolyte interface
ïWhen a semiconductor comes into contact with a liquid,
to maintain electrostatic equillibrium
ïThere will be a charge transfer between the
semiconductor and liquid phase,if formal redox potential
of redox species lies inside semiconductor band gap.
34. ïAt thermodynamic eqilibrium, the fermi level of
semiconductor and the formal redox potential of redox
species and between interface semiconductor.
ïThis introduce n-type semiconductor and p-type
semiconductor.
ïThis semiconductor used as photovoltaic device similar to
solid state p-n junction devices.
ïBoth n and p type semiconductor can used as photovoltaic
devices to convert solar energy into electrical energy and
are called photoelectrical cells
35. ï Boielectrochemistry
ïIt is branch of electrochemistry and biophysical
chemistry concerned with topics like cell electron-
proton transport, cell membrane potentials and
electrode reactions of redo enzymes.
ïBioelectrochemistry is a science at the many junctions
of sciences.
36. Nanoelectrochemistry
ïNanoelectrochemistry is a branch of electrochemistry
that investigates the electrical and electrochemical
properties of materials at the nanometer size regime.
ïNanoelectrochemistry plays significant role in the
fabrication of various sensors, and devices for detecting
molecules at very law concentrations.
37. ïThe term electrochemical nanostructuring can be used
to mean different things.
ïThis term is employed to refer to generation at will of
nanostructure on electrode surface, involving a given
positioning with a certain precision
ïThe term nanostructure is used to describe the
generation of nanometric patterns with move or less
narrow size distribution and a periodic or random
ordering on the surface.
ïBut without control on the spatial location of the
nanostructure.
38. Application of electrochemistry
ïThere are various extremely important electrochemical
processes in both nature and industry.
ïThe coating of objects with metals or metal oxides
through electro deposition and the detection of alcohol in
drunken drivers through the redox reaction of ethanol.
ïDiabetes blood sugar meters measure the amount of
glucose in the blood through its redox potential.
39. ïThe generation of chemical energy through
photosynthesis in inherently an electrochemical process.
ïProduction of metals like aluminium and titanium from
their ores.
ï For Photo electrochemistry
ïArtificial photosynthesis
ïRegenerative cell or Dye-sensitized cell
ïPhoto electrochemical splitting of water
40. ï For Boielectrochemistry
ïSome of different experimental techniques that can be
used to study bioelectrochemical problems.
ïAmpermetic of biosensors
ïBiofuel cells
ïBioelectrosynthesis