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ELECTROCHEMISTRYELECTROCHEMISTRY
CHEMICAL CHEMICAL SUBSTANCESSUBSTANCES
ELECTROLYTES NON-ELECTROLYTES
Substances that can conduct electricity when they are in molten state or aqueous and undergo chemical changes
Substances that cannot conduct electricity either in molten state or aqueous
Example:
Ionic substances
(i) Dilute acid solution
(ii) Dilute alkaline solution
(iii) Molten salts
(iv) Aqueous salt solution
Example:
Covalent substances
(i) Naphthalene
(ii) Sugar solution
(iii) Latex
(iv) Hydrogen chloride in organic solvents
Heat
Molten lead (II) iodide
BulbCarbon electrodes
Heat
Solid lead (II) iodide
Carbon electrodes
Bulb
………….
…. ..… ………..…. ….
… ……….…. …. …. ….…. …. ….….….….….
switchswitch
•Do not conduct electricity
•This is because the ions are held in a fixed crystal lattice.
•They are held with the strong electrostatic forces of attraction
•Do not freely move
I - Pb 2+
Pb 2+ Pb 2+ I -I -
I -
I -I - Pb 2+
Pb 2+
Pb 2+
Pb 2+
Solid lead (II) iodide
IN A SOLID STATEIN A SOLID STATE
Molten lead (II) iodide
I -
Pb 2+
Pb 2+ Pb 2+
I -I -
•Can conduct electricity
•This is because the presence of moving ions. The ions are free to move in the molten or aqueous solution
IN A MOLTEN STATEIN A MOLTEN STATE
ELECTROLYTES AND NON ELECTROLYTES AND NON ELECTROLYTESELECTROLYTES
Classify the following chemicals into electrolytes or non-Classify the following chemicals into electrolytes or non-electrolyteselectrolytes
Potassium chloride, KCl solutionPotassium chloride, KCl solution Molten lead (II) bromide, PbBrMolten lead (II) bromide, PbBr22
Glucose solutionGlucose solution TrichloromethaneTrichloromethane Molten zinc oxide, ZnOMolten zinc oxide, ZnO Sodium chloride, NaCl solutionSodium chloride, NaCl solution Ammonia in tetrachloromethaneAmmonia in tetrachloromethane
A process of A process of breaking downbreaking down the chemical the chemical compounds into their constituent elements using compounds into their constituent elements using electric currentelectric current
Example:Example:Molten aluminium oxide (I) aluminium (s) + oxygen (g)
Copper (II) chloride (aq) copper (s) + chlorine (g)Electric current
Electric current
ELECTROLYSISELECTROLYSIS
ELECTROLYTIC CELLELECTROLYTIC CELL
Electrolyte
e-
e- e-
e-
Electrode Electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
- +
Anion Cation
The set of apparatus needed to conduct The set of apparatus needed to conduct electrolysiselectrolysis
It consists of a It consists of a batterybattery, an , an electrolyteelectrolyte, and , and two two electrodeselectrodes (anode and cathode) (anode and cathode)
AnodeAnode - the electrode which is connected to the - the electrode which is connected to the positive terminal of an electric source in the positive terminal of an electric source in the electrolytic cellelectrolytic cell
CathodeCathode - the electrode which is connected to - the electrode which is connected to the negative terminal of an electric source in the the negative terminal of an electric source in the electrolytic cellelectrolytic cell
ELECTROLYTIC CELLELECTROLYTIC CELL
ANODEANODE
(POSITIVE ELECTRODE)(POSITIVE ELECTRODE)
CATHODE
(NEGATIVE ELECTRODE)(NEGATIVE ELECTRODE)
Anions (negative ions)Anions (negative ions) will be pulled towards will be pulled towards the anode (positive the anode (positive electrode)electrode)
Cations (positive ions)Cations (positive ions) will will be pulled towards the be pulled towards the cathode (negative cathode (negative electrode)electrode)
At the anode, anions At the anode, anions will be discharged by will be discharged by releasingreleasing the electrons the electrons to the anodeto the anode
At the cathode, cations will At the cathode, cations will be discharged by be discharged by receivingreceiving the electrons the electrons from the from the cathodecathode
During electrolysisDuring electrolysis::
ELECTROLYSIS OF MOLTEN ELECTROLYSIS OF MOLTEN COMPOUNDSCOMPOUNDS
QUESTIONSQUESTIONS
(a) Molten zinc chloride (I)
(b) Molten aluminium (III) bromide
(c) Molten zinc (II) iodide
(d) Molten lead (II) oxide Electric current
Electric current
Electric current
Electric current
Example 1Example 1
Molten Potassium Iodide, KI
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
The ions that presents in electrolyte are:
(i) Anion:
(ii) Cation:
Example 2Example 2
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
The ions that presents in electrolyte are:
(i) Anion:
(ii) Cation:
Molten zinc oxide, ZnO
Example 3Example 3
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
The ions that presents in electrolyte are:
(i) Anion:
(ii) Cation:
Molten lead (II) bromide, PbBr2
Example 4Example 4
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
The ions that presents in electrolyte are:
(i) Anion:
(ii) Cation:
Molten lead (II) oxide, PbO
Example 5Example 5
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
The ions that presents in electrolyte are:
(i) Anion:
(ii) Cation:
Molten zinc (II) chloride, ZnCl2
ELECTROLYSIS OF MOLTEN ELECTROLYSIS OF MOLTEN COMPOUNDCOMPOUND
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
The ions that presents in electrolyte are:
(i) Anion:
(ii) Cation:
Molten lead (II) bromide, PbBr2
Molten lead (II) bromide
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
…… ……………… …..
…. ….. …… … ….
.. . …….. …… … …
……………………………………...
Pb2+
Pb2+
Pb2+
Pb2+
Br-
Br-
Br-
Br-
ELECTROLYSIS OF MOLTEN ELECTROLYSIS OF MOLTEN COMPOUNDCOMPOUND
PbPb2+2+ are attracted to the cathode are attracted to the cathode BrBr-- are attracted to anode are attracted to anode
BrBr-- discharge by releasing electrons to the discharge by releasing electrons to the anodeanode
CATHODECATHODE
(NEGATIVE ELECTRODE)(NEGATIVE ELECTRODE)
ANODEANODE
(POSITIVE ELECTRODE)(POSITIVE ELECTRODE)
Br- Br + e-
Neutral atoms form and combine to form neutral bromine molecules
Br + Br Br2 (g)
The half reaction at anode can be represented by the half equation
2Br- (l) Br2 (g) + 2e-
Pb2+ discharge by receiving electrons (provided by the battery) at the cathode to form neutral lead atoms
Pb2+(l) + 2e- Pb (s)
The half reaction at cathode can be represented by the half equation
The Half Equation:
Cathode:
Anode:
Overall Equation:
2Br- (l) Br2 (g) + 2e-
Pb2+(l) + 2e- Pb (s)
Pb2+(l) + 2Br- (l) Pb(s) + Br2 (g)
Write the half equation and the overall Write the half equation and the overall equation for the electrolysis of these equation for the electrolysis of these molten compounds :molten compounds :
(A) Molten potassium iodide, KI(A) Molten potassium iodide, KI
(B) Molten zinc (II) chloride, ZnCl(B) Molten zinc (II) chloride, ZnCl22
(C) Molten lead (II) oxide, PbO(C) Molten lead (II) oxide, PbO
ELECTROLYSIS OF AQUEOUS ELECTROLYSIS OF AQUEOUS SOLUTIONSOLUTION
Water molecules in an aqueous solution can slightly dissociate to produce H+ and OH-
H2O H+ (aq) + OH-(aq)
So, aqueous solution contains H+ and OH- and electrolyte ions
Examples:
Aqueous SolutionAqueous Solution
Ions presentIons present
AnionAnion CationCation
NaCl solutionNaCl solution ClCl-- , OH , OH-- NaNa++ , H , H++
CuSOCuSO44 solution solution
HNOHNO33 solution solution
If they are more than one cations or anions If they are more than one cations or anions attracted, the choice of ion to be discharged attracted, the choice of ion to be discharged
depends on :depends on :
Positions of the ions Positions of the ions in the in the electrochemical serieselectrochemical series
Types of Types of electrodeselectrodes
Concentration of ionsConcentration of ions in the electrolytein the electrolyte
Electrochemical Series (pg.101)Electrochemical Series (pg.101)
CATIONSCATIONS
KK + + NaNa++
CaCa2+2+
MgMg2+2+
Al Al 3+3+
ZnZn2+2+
FeFe2+2+
SnSn2+2+
PbPb2+2+
HH++
CuCu2+2+
AgAg++
Tendency to discharge increases
ANIONSANIONS
FF--
SOSO4422--
NONO33--
ClCl--
BrBr--
II--
OHOH--
Positions of the ions Positions of the ions in the electrochemical seriesin the electrochemical series
Copper (II) chloride solution, CuCl2
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
H+
Cu2+
Cu2+
H+
Cl-
Cl-OH-
OH-
Positions of the ions Positions of the ions in the electrochemical seriesin the electrochemical series
Observation Observation andand
ProductProduct
HH++ , Cu , Cu2+2+
CuCu2+2+are preferred to be dischargedare preferred to be discharged
(Cu(Cu2+ 2+ is below His below H++ in the ES) in the ES)
OHOH-- , Cl , Cl- -
OHOH-- are preferred to be discharged are preferred to be discharged
(OH(OH-- is below Cl is below Cl- - in the ES)in the ES)
Ions that are Ions that are attractedattracted
CathodeCathodeAnodeAnode
Bubbles of gas, OBubbles of gas, O22
is releasedis releasedBrown solid, Cu is formedBrown solid, Cu is formed
Half Half equationequation
4OH4OH- - (aq) 2H(aq) 2H22O (l) + OO (l) + O22 (g) (g)
+ 4 e+ 4 e--
CuCu2+ 2+ (aq) + 2e(aq) + 2e-- Cu (s) Cu (s)
Concentration of ions in Concentration of ions in electrolyte solutionselectrolyte solutions
Concentration of ions in electrolyte solution also Concentration of ions in electrolyte solution also can affects the choice of ions to be dischargedcan affects the choice of ions to be discharged
An ion that is An ion that is more concentratedmore concentrated is preferably is preferably dischargeddischarged
AnodeAnode – the ions to be discharged is – the ions to be discharged is determined by determined by the concentration of ionsthe concentration of ions
CathodeCathode – the ions to be discharged is – the ions to be discharged is determined by determined by the position of the ion in the the position of the ion in the E.SE.S
Concentration of ions in Concentration of ions in electrolyte solutionselectrolyte solutions
Concentrated copper (II) chloride solution, CuCl2
e-
e- e-
e-
Carbon electrode
Carbon electrode
- (cathode)+ (anode)
Cu2+
H+Cl-
OH-
Concentration of ions in Concentration of ions in electrolyte solutionselectrolyte solutions
Observation Observation and and
ProductProduct
HH++ , Cu , Cu2+2+
CuCu2+2+are preferred to be dischargedare preferred to be discharged
(Cu(Cu2+ 2+ is below His below H++ in the ES) in the ES)
OHOH-- , Cl , Cl--
ClCl-- are preferred to be discharged are preferred to be discharged
(Cl(Cl- - is more concentrated) is more concentrated)
Ions that are Ions that are attractedattracted
CathodeCathodeAnodeAnode
Yellow bubbles gas, ClYellow bubbles gas, Cl22
is releasedis released
Brown solid, Cu is formedBrown solid, Cu is formed
Half Half equationequation
2Cl2Cl- - (aq) Cl(aq) Cl22 (g) + 2 e (g) + 2 e--CuCu2+ 2+ (aq) + 2e(aq) + 2e-- Cu (s) Cu (s)
Types of ElectrodesTypes of Electrodes
Silver nitrate, AgNO3 solution
e-
e- e-
e-
Silver plate Carbon electrode
- (cathode)+ (anode)
Ag+
AgAg+
Types of ElectrodesTypes of Electrodes
AgAg+ + (aq) + e(aq) + e-- Ag (s) Ag (s)
Observation Observation and and
ProductProduct
AgAg++ receives one electron to receives one electron to form metal atomsform metal atoms
Ag atom releases one electron to form Ag atom releases one electron to form AgAg++
IonsIons
CathodeCathodeAnodeAnode
The silver plate corrodesThe silver plate corrodes Grey silver solid, Ag is Grey silver solid, Ag is formedformed
Half Half equationequation
Ag (s) AgAg (s) Ag+ + (aq) + e(aq) + e--
Exercises Exercises
Electrolysis of copper (II) sulphate, CuSOElectrolysis of copper (II) sulphate, CuSO44, solution , solution
using carbon electrodesusing carbon electrodes
AnodeAnode CathodeCathode
Ions that are Ions that are attractedattracted
Ion that are Ion that are prefer to be prefer to be dischargeddischarged
ObservationObservation
ProductProduct
Half equationHalf equation
ExercisesExercises
Electrolysis of concentrated potassium chloride, KCl, Electrolysis of concentrated potassium chloride, KCl, solution using carbon electrodessolution using carbon electrodes
AnodeAnode CathodeCathode
Ions that areIons that are
attractedattracted
Ion that are Ion that are prefer to be prefer to be dischargeddischarged
ObservationObservation
ProductProduct
Half equationHalf equation
ExercisesExercises
Electrolysis of nickel (II) sulphate, NiSOElectrolysis of nickel (II) sulphate, NiSO44, solution , solution
using nickel plate as anode and cathodeusing nickel plate as anode and cathode
AnodeAnode CathodeCathode
Half equationHalf equation
ObservationObservation
ProductProduct
Factors that influence electrolysis Factors that influence electrolysis of aqueous solutions of aqueous solutions
TYPES OF ELECTRODESTYPES OF ELECTRODES
POSITION OF IONS POSITION OF IONS
IN THE ELECTROCHEMICAL IN THE ELECTROCHEMICAL SERIESSERIES
CONCENTRATION OF IONS CONCENTRATION OF IONS
IN THE ELECTROLYTE IN THE ELECTROLYTE SOLUTIONSOLUTION
USES OF ELECTROLYSISUSES OF ELECTROLYSIS
IN INDUSTRIESIN INDUSTRIES
Reacts with a Reacts with a carbonate metal metal to form carbon to form carbon dioxide gas (COdioxide gas (CO22),water ),water
(H(H22O) and saltO) and salt
ELECTROPLATING ELECTROPLATING OF METALSOF METALS
EXTRACTIONEXTRACTION OF METALS OF METALS
PURIFICATIONPURIFICATION OF OF METALSMETALS
Extraction of MetalsExtraction of Metals Electrolysis can be used to extract metals from Electrolysis can be used to extract metals from
their orestheir ores Reactive metals that are Reactive metals that are more reactivemore reactive than C than C
such as (K, Na, Ca, Mg, Al) cannot be such as (K, Na, Ca, Mg, Al) cannot be extracted through extracted through heatingheating of their metal of their metal oxides with Coxides with C
They need to be extracted from their molten They need to be extracted from their molten ores using the ores using the electrolysis processelectrolysis process
In this process:In this process:
ElectrolyteElectrolyte The molten oreThe molten ore
AnodeAnode Carbon electrodeCarbon electrode
CathodeCathode Carbon electrodeCarbon electrode
Example:Example:
Extraction of aluminium from electrolysis Extraction of aluminium from electrolysis of molten aluminium oxide, Alof molten aluminium oxide, Al22OO33
Purification of MetalsPurification of Metals Metals that have been extracted from their Metals that have been extracted from their
ores are normally not pure. They contains ores are normally not pure. They contains impurities which need to be removedimpurities which need to be removed
These metals can be purified by electrolysis These metals can be purified by electrolysis processprocess
In the purification processIn the purification process
ElectrolyteElectrolyte The solution that contains The solution that contains
the metal ionsthe metal ions
AnodeAnode The impure metal plateThe impure metal plate
CathodeCathode The pure metal plateThe pure metal plate
Example:Example:
Purification of copperPurification of copper
Electroplating of MetalsElectroplating of Metals Many types of metals can be plated with other Many types of metals can be plated with other
metals through electrolysis.metals through electrolysis. The aim of metal plating through electrolysis The aim of metal plating through electrolysis
includes:includes:
(i) making the metal more (i) making the metal more resistantresistant to to corrosioncorrosion
(ii) making the metal appear more (ii) making the metal appear more attractiveattractive In the electroplating processIn the electroplating process
ElectrolyteElectrolyte The solution which contains The solution which contains ions of plating metalions of plating metal
AnodeAnode Plating metalPlating metal
CathodeCathode Metal to be platedMetal to be plated
Example:Example:
Electroplating of a iron spoon with copper Electroplating of a iron spoon with copper metalmetal
Copper (II) Copper (II) sulphate sulphate solution solution
ELECTROLYTIC CELLELECTROLYTIC CELL
e-
e- e-
e-
CarbonCarbon
electrodeelectrodeCarbonCarbon
electrode electrode
- (cathode) + (anode)
VOLTAIC CELLVOLTAIC CELL
CuCu
Copper (II) Copper (II) sulphatesulphate
V
e-
e- e-
e-
- (anode)- (anode) + (cathode)+ (cathode)
ZnZn
Zn (s) ZnZn (s) Zn2+ 2+ (aq) + 2e(aq) + 2e-- CuCu2+ 2+ (aq) + 2e(aq) + 2e- - Cu Cu (s)(s)
VOLTAIC CELLVOLTAIC CELL
Also known as Also known as galvanic cellgalvanic cell Has Has two different metalstwo different metals which are immersed which are immersed
into an electrolyte and connected by wireinto an electrolyte and connected by wire Produces electrical energy from the chemical Produces electrical energy from the chemical
reactions occurring inside the cellreactions occurring inside the cell
Example : Daniell cellExample : Daniell cell
Chemical energy electrical energyChemical energy electrical energy
DANIELL CELLDANIELL CELL
V
Dilute HDilute H22SOSO44
(Salt bridge)(Salt bridge)
Zn (-)Zn (-) Cu (+)Cu (+)
CuSOCuSO44
solutionsolution
ZnSOZnSO44 solution solution
(Anode)(Anode) (Cathode)(Cathode)
e- e-
e- e-
Zn (s) ZnZn (s) Zn2+ 2+ (aq) + 2e(aq) + 2e-- CuCu2+ 2+ (aq) + 2e(aq) + 2e- - Cu Cu (s)(s)
SALT BRIDGESALT BRIDGE Can be made from any electrolyte that does not Can be made from any electrolyte that does not
react with the electrodes in Daniell Cellreact with the electrodes in Daniell Cell Function :Function :
(i) to allow the flow of the ions so the electric (i) to allow the flow of the ions so the electric current is completedcurrent is completed
ExampleExample::
(i) diluted H(i) diluted H22SOSO44
(ii) sodium nitrate, NaNO(ii) sodium nitrate, NaNO3 3 solutionsolution
(iii) Potassium chloride solution, KCl(iii) Potassium chloride solution, KCl
DANIELL CELLDANIELL CELL
V
Porous Porous pot pot contains contains ZnSOZnSO44
Zn (-)Zn (-) Cu (+)Cu (+)
CuSOCuSO4 4
solutionsolution
(Anode)(Anode)(Cathode)(Cathode)
e- e-
e- e-
Reactivity SeriesReactivity Series
KK NaNaCaCaMgMgAl Al ZnZnFeFeSnSnPbPbHH
CuCuAgAg
METALSMORE
ELECTROPOSITIVE
(negative terminal)
MORE ELECTRONEGATIVE
(positive terminal)
Anode and CathodeAnode and Cathode
AnodeAnode – the electrode where the process of – the electrode where the process of donation of electronsdonation of electrons takes place takes place
CathodeCathode – the electrode where the process of – the electrode where the process of receiving of electronsreceiving of electrons takes place takes place
Negative terminal – Cathode
Positive terminal - Anode
Negative terminal – Anode
Positive terminal - Cathode
ELECTROLYTIC CELLELECTROLYTIC CELL VOLTAIC CELLVOLTAIC CELL
ELECTROCHEMICAL SERIESELECTROCHEMICAL SERIES
Electrochemical Series (pg.101)Electrochemical Series (pg.101)
CATIONSCATIONS
KK + + NaNa++
CaCa2+2+
MgMg2+2+
Al Al 3+3+
ZnZn2+2+
FeFe2+2+
SnSn2+2+
PbPb2+2+
HH++
CuCu2+2+
AgAg++
Tendency to discharge increases
ANIONSANIONS
FF--
SOSO4422--
NONO33--
ClCl--
BrBr--
II--
OHOH--
ELECTROCHEMICAL ELECTROCHEMICAL SERIESSERIES
An arrangement of metals, based on the tendency of each metal atom to donate electrons
The higher the position of a metal in the electrochemical series:
ELECTROCHEMICAL SERIESELECTROCHEMICAL SERIES
More electropositiveMore electropositive The The greatergreater the tendency the tendency of the metal atoms of the metal atoms to to donate electronsdonate electrons
PRINCIPLES DURING CONSTRUCTING PRINCIPLES DURING CONSTRUCTING THE ELECTROCHEMICAL SERIESTHE ELECTROCHEMICAL SERIES
Potential differences Potential differences between two metals in the between two metals in the voltaic cellvoltaic cell
Ability of a metal to Ability of a metal to displace another metal displace another metal from its salt solutionfrom its salt solution
The value of the potential difference of a simple voltaic The value of the potential difference of a simple voltaic cell is affected by the cell is affected by the position of the metalsposition of the metals in the in the electrochemical serieselectrochemical series
When two When two different metalsdifferent metals are immersed in an electrolyte are immersed in an electrolyte solution, a solution, a potential differencepotential difference is generated is generated
The The largerlarger the value of the cell voltage is produced the value of the cell voltage is produced
The The furtherfurther the two metals in the electrochemical series the two metals in the electrochemical series
Potential differences between two Potential differences between two metals in the voltaic cellmetals in the voltaic cell
Potential differences between two Potential differences between two metals in the voltaic cellmetals in the voltaic cell
The metal that is The metal that is more more electropositiveelectropositive
Located Located higherhigher in the in the electrochemical serieselectrochemical series
Act as the Act as the negative terminalnegative terminal
The metal that is The metal that is less less electropositiveelectropositive
Located Located lowerlower in the in the electrochemical serieselectrochemical series
Act as the Act as the positivepositive terminal terminal
Potential differences between two Potential differences between two metals in the voltaic cellmetals in the voltaic cell
Mg
Zn
Pb
Cu
Ag
3.0 V1.1 V
0.4 V
0.5 V
Predict the negative terminal, positive terminal and cell voltage of the following voltaic cell
(a) Magnesium and silver (c) zinc and lead
(b) Magnesium and zinc (d) zinc and silver
Metal DisplacementMetal Displacement
A metal that is more electropositive can displace another metal which is less electropositive from its salt solution
This reaction – displacement reaction
A metal that is located higher in the electrochemical series can displace another metal which is located lower in the electrochemical series from its salt solution
Metal DisplacementMetal Displacement
Example:
Zinc, Zn can displace copper, Cu, from copper (II) nitrate, Cu(NO3)2
solution
Zn (s) + Cu(NO3)2 (aq) Zn(NO3)2 (aq) + Cu (s)
• Zn is more electropositive than copper
• Zn can displace Cu from copper (II) nitrate, Cu(NO3)2 solution
• The zinc, Zn, will dissolve and brown copper solid, Cu, will form
Metal displaced
IMPORTANCE OF THE IMPORTANCE OF THE ELECTROCHEMICAL ELECTROCHEMICAL
SERIESSERIES
Reacts with a Reacts with a carbonate metal metal to form carbon to form carbon dioxide gas (COdioxide gas (CO22),water ),water
(H(H22O) and saltO) and salt
It can determined the terminals of voltaic cells
It can determined the cell voltage for a pair of
metals
It can predicted the potential of a metal to displace another metal
from its solution