Unit-III-ELECTROCHEMICAL STORAGE DEVICES.ppt

Batteries -Introduction – Types of Batteries – discharging and charging of battery - characteristics of battery –battery rating- various tests on battery- – Primary battery: silver button cell- Secondary battery :Ni-Cd battery-modern battery: lithium ion battery-maintenance of batteries-choices of batteries for electric vehicle applications.
Fuel Cells: Introduction- importance and classification of fuel cells - description, principle, components, applications of fuel cells: H2-O2 fuel cell, alkaline fuel cell, molten carbonate fuel cell and direct methanol fuel cells.

1. 10-Jun-24
Prepared by
Mrs.K.Krishnaveni
Assistant Professor
Department of Chemistry
Kongu Engineering College
Perundurai, Erode
Unit –III –Electrochemical Storage Devices

2. UNIT -III
ELECTROCHEMICAL STORAGE DEVICES
Batteries -Introduction –Types of Batteries –discharging and charging of battery -
characteristics of battery –battery rating-various tests on battery-–Primary battery:
silver button cell-Secondary battery :Ni-Cd battery-modern battery: lithium ion battery-
maintenance of batteries-choices of batteries for electric vehicle applications.
Fuel Cells: Introduction-importance and classification of fuel cells -description,
principle, components, applications of fuel cells: H
2-O
2fuel cell, alkaline fuel cell,
phomolten carbonate fuel cell and direct methanol fuel cells.

3. Introduction:
oThe function of Batteries / cells is the conversion of chemical energy into electrical energy.
It is made up of two electrodes (anode & cathode) and electrolyte solution
Definition:
Cell is an arrangement of two electrodes dipped into a solution of electrolyte or electrolytes.
oCathode –Positive terminal –Electrochemical reduction occurs (gain electrons)
oAnode –Negative terminal –Electrochemical oxidation occurs (lose electrons)
oElectrolytes –Allow Ions to move between electrodes
oTerminals –Allows Current to flow out of the battery to
perform work
CELLS

4. List of invented cells / Batteries
Alessandro Volta invented the first true battery

5. oDue to increasing human activity in technology, a number of battery dependent appliances
have come into existence.
oIt is used in wrist watches, electric calling bells, space vehicles and missile firing units.
Importance of Cells / Batteries /
There are two types of cells, 1. Electrolytic cell 2. Electrochemical cell
Types of Cells
-Electricalenergyisusedtobringaboutthechemicalreaction.
At anode : Oxidation takes place
(Ni → Ni
2+
+2e
-
)
At cathode : Reduction takes place
( Ni
2+
+2e
-
→ Ni )

6. oElectrical energy is generated due to chemical reactions, which takes place inside the cells
oExamples: Daniel cell, Zn / ZnSO
4// CuSO
4/ Cu
At anode,
Zn → Zn
2+
+2e
-
(Oxidation)
At cathode,
Cu
2+
+ 2e
-
→ Cu (Reduction)
The overall reaction,
Zn + Cu
2+
→ Zn
2+
+ Cu

7. Abatteryisanarrangementofseveralelectrochemicalcellsconnectedinseries/
paralleltogetrequiredamountofelectricalenergy.
Thebatterycontainsseveralanodesandcathodes.
BATTERIES
Criteria for any cells to be commercial cells
Should be cheap
Light weight and portable
should have long life cycle and high self life.
should be continuous and constant sources of EMF over a long interval of time.
It should be a rechargeable unit.

8. Selection of battery depends on the conditions of working, the suitability of a battery
depends on the following characteristics:
oType
oVoltage
oDischarge curve
oCapacity
oEnergy density
oSpecific energy density
oPower density
oTemperature dependence
oService life
oPhysical requirements
oCharge/discharge cycle
oCycle life
oCost
oAbility to deep discharge
oApplication requirements

12. Cyclelife:
oItisdefinedasnumberoftimesthedischargingandchargingoperationscanbealternated
tillsuchtimeitperformsasdesigned.
oItisapplicableonlytosecondarycells.TheEMFofcelldecreaseduringdischarging.
oAgoodcellshouldhavehighcyclelife.
osometimescyclelifewouldbelowerthanexpectedleveldueto,
Theactivematerialsattheelectrodesmaywhitheroffduetorapidchargingconditions.
Maybeirregulardepositionoftheproductsduringdischarging.
Overcharging,thecorrosionmayoccur.
Shelflife:
Agoodbatteryshouldpossessalongshelflife.
Self-discharge:
oItisdefinedasthelossofactivematerialsofthecellduetolocalizedactiononthe
electrodeeventhecellisnotindischargemode.
oLongerthelifeself-discharge,goodbattery

13. Discharging:
The electrons liberated at the anode flow to
the cathode through the external wire and take
part in the reduction. This process in which
spontaneous redoxreaction occurs is called
discharging.
During discharging , the active materials are
converted into inactive materials.
The cell becomes inactive once the active
material is consumed.
External energy < Cell energy
Charging:
The cell reaction is reversed if the external
current is passed in the reverse direction.
This process of conversion of an inactive
material back into active materials in a cell is
called charging.
It is a non-spontaneous process.
External energy > Cell energy
DischargingandChargingofabattery
oA cell is a battery that is packed that active materials at anode and cathode, redox reaction occur spontaneously.

14. The batteries are classified into
oPrimary batteries
oSecondary batteries
1. Primary battery (Non-rechargeable)
The electrode and its reaction cannot be reversed by passing electrical energy externally.
During discharging the chemical compounds are permanently changed and electrical energy
is released until the original compounds are completely exhausted.
In such batteries the reaction occurs only once and it is not rechargeable
Lower discharge rate than secondary batteries
Examples: Dry Leclanchecell -Zinc Carbon –Used in flashlights, toys
Heavy Duty Zinc Chloride –Used in radios, recorders
Alkaline –Used in all of the above
Lithium –Used in photoflash
Silver Mercury Oxide –Used in Hearing aid, watches, calculators,
Silver button cell–Small devices like above
Types of Batteries

15. 2. Secondary battery (Chargeable)
oThe electrode reactions can be reserved by passing electrical energy externally.
oDuring discharging the chemical compounds which are changed can be reconstituted by
the application of an electrical potential between the electrodes –“electrochemical
reaction is reversible”
oThey can be recharged by passing electrical current and used endlessly.
oUsed when short periods of storage are required
oHigher discharge rate than primary batteries.
oThus such cells can be Rechargeable and used many times.
oExamples: Lead Acid Battery
Nickel Cadmium Battery
Nickel Metal Hydride Battery
Lithium Ion Battery

17. Primary battery -Silver button battery
What is a Button battery?
oAButton battery or button cellis a small single cellbattery,
oCylindrically shaped about 5 to 25mm in diameter and 1 to 6mm high
Structure
Button batteries are formed by compacting metals and metal oxides on either side of an
electrolyte-soaked separator.
The unit is then placed in a 2-part metal casing held together by a plastic grommet
The grommet electrically insulates the anode from the cathode.
The metal undergoes oxidation on one side of the separator,
while the metal oxide is reduced to the metal on the other side,
producing a current when a conductive path is provided.
Uses: In small portable electronic devices -wrist watches, pocket calculators, artificial
cardiac pacemakers, implantable cardiac defibrillators, hearing aids, toys, etc

18. Importance
oButton-typesilveroxidebatteriesgiveshigh-energyper
unitvolumeandstableoperatingvoltage.
oAlso,itisdesignedtousezeromercury.
oMaxellisthefirstcompanyinJapantosuccessfully
marketbutton-typesilveroxidebatteries.
Construction and working:
oThis cell consist of silver oxide as cathode
and zinc metal as the anode.
oThese electrodes are separated by
semi-permeable membranes and
pottasiumhydroxide and sodium hydroxide
is used as an electrolyte
oCellrepresentation
Zn,ZnO/Electrolyte/Ag
2O,Ag

19. Cell reactions:
At the anode : Zn + 2OH
-
→ ZnO+ H
2O + 2e
-
At the cathode : Ag
2O + H
2O +2e
-
→ 2Ag + 2OH
-
Overall cell reaction : Zn + Ag
2O → ZnO+ 2Ag
The cell gives a voltage of 1.3-1.5 V.
Advantages:
oDuring discharge, supplies a stable voltage until the end of the discharge life.
oA silver oxide battery’s gives twice the amount of energy capacity as button-type alkaline
batteries.
oDepending on the composition of the electrolyte, two models are available; a low-drain type
(SW type) for analogwatches and a high-drain type (W type) for multi-function watches (which
incorporate an alarm and a light), medical equipment.
oDesigned without using mercury and lead and also long lasting, superior leakage -resistant
characteristics

21. oRechargeablealkalinebattery
oDuringcharginganddischarging,nolossofproducts
oActivematerialsusedinthebatterysystemare,
Anode :Cadmiumasamixtureofmetal,oxideorhydroxide
Cathode:Nickeloxyhydroxide
Electrolyte:AquousKOH
oCellrepresentation
Cd,Cd(OH)
2/KOH(aq)/Ni(OH)2,NiO(OH)
Construction
oIt consists of cadiumanode and a metal grid
containing a paste of NiO(OH)acting as a cathode
oElectrolyte in the cell is KOH it is
Nickel-Cadmium batteries (NICAD)/ Secondary battery

22. Working:
During Discharging
When the NICAD battery operates, at the anode
cadmium is oxidised to Cd
2+
ions and insoluble Cd(OH)
2is formed
Cell reaction
At anode: Oxidation takes places at cadmium
Cd → Cd
2+
+ 2e
-
Cd
2+
+ 2OH
-
→ Cd(OH)
2
At cathode: Reduction of nickel oxyhydroxidetakes
place in this reaction
2NiO(OH) + 2H
2O + 2e
-
→ 2Ni(OH)
2+ 2OH
-
Net cell reaction
Cd + 2NiO(OH) + 2H
2O → Cd(OH)
2 + 2Ni(OH)
2

23. During Charging
oWhen current is passed in the opposite direction, the electrode reaction gets reversed.
oAs a result, cadmium gets deposited on the anode and
NiO(OH) gets deposited on the cathode.
At cathode:
Cd(OH)
2→ Cd
2+
+ 2OH
-
Cd
2+
+ 2e
-
→ Cd
At anode:
2Ni(OH)
2+ 2OH
-
→ 2NiO(OH) + 2H
2O + 2e
-
Net cell reaction
Cd(OH)
2+ 2Ni(OH)
2→ Cd + 2NiO(OH) + 2H
2O
Thecellvoltageofbatteryis1.4V,whichisirrespectiveofthesizeofelectrodes.

24. Applications:
Ni-Cdbatteriesmaybeusedindividuallyorassembledintobatterypacks
containingtwoormorecells.
Ni-Cdbatteriesareusedincordlessandwirelesstelephones,emergencylighting
andotherapplications.
Withalowinternalresistance,theycansupplyahighsurgecurrent.Thismakes
themafavourablechoiceforremotecontrolledmodelairplanes,boats,carsand
cameraflashunits.

25. Advantages:
Delivershighcurrentoutput
Haveabilitytodeliverfullpoweroutputuntilendofcycle
Ittoleratesovercharging
Itwithstandsupto500cyclesofcharging
Ithaslongerlife(lessthan20years)thanleadstoragecell
Operateinarangeoftemperatures.
Nogasevolutionoccursattheactiveelectrodes.
Theyhavelowinternalresistance.
Likeadrycell,itcanbepackedinasealedcontainer.
Disadvantages:
oCadmiumisnotaneco-friendlymaterial-Materialsaretoxicandtherecycling
infrastructureforlargernickel-cadmiumbatteriesisverylimited
oLesstolerancetowardstemperatureascomparedtootherbatteries.
oItisthreetofivetimesmoreexpensivethanlead-acid
oSelfdischargeupto10%inaday.

26. Fuel cells are electrochemical cells that convert chemical
energy from a fuel into electricity through catalytically
activated redox reactions.
Conventionallyenergyisobtainedbythecombustionof
fossilfuel.
Theconversionofheatintoelectricalenergyinvolvesa
numberofstepsandthereislossofenergyateverystep.
Efficiencyoftheprocessisaround40%.
i.e.,InFuel(Gasoline,Dieselandetc.)
ChemicalEnergy→ HeatEnergy→MechanicalEnergy
→ElectricalEnergy
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Fuel Cells
Fuel + Oxygen Oxidation products + Electricity

27. Toovercomethese,thedevicefuelcellsweredemonstratedwhichareaclean,
efficient,reliable,andquietsourceofpower.Fuelcellsdonotneedtobeperiodically
rechargedlikebatteries,butinsteadcontinuetoproduceelectricityaslongasafuel
sourceisprovided.
InFuelcellsthechemicalenergyisdirectlyconvertedtoelectricalenergy.
ChemicalEnergy→ElectricalEnergy
Thisdirectionconversionofchemicalenergyintoelectricalenergyhas100%
efficiency.
Fuelcellsareusedtodayinarangeofapplications,fromprovidingpowertohomes
andindustries,keepingcriticalfacilitieslikehospitals,grocerystores,andmovinga
varietyofvehiclesincludingcars,buses,trucks,trains,andmore.
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28. 10-Jun-24

29. Fuel Cells
Thebasicprincipleofafuelcellisthesameasthatof
electrochemicalcells.
SinglefuelcellgeneratesonlylittleDCandhencemanyfuel
cellsareassembledintoastack.
Ithasaseparatefuel-oxidantsystemthatproduces
electrochemicalreactioninwhichthefuelisoxidizedatthe
anode.
Likeotherelectrochemicalcell,thefuelcellsalsoconsistofan
electrolyteandtwoelectrodes.
However,themaindifferenceinthecellfunctionisthat
electrochemicalenergyisprovidedbyafuelandanoxidantis
storedoutsidethecellwhereelectrochemicalreactiontakesplace.
Hence,fuelcellscanproduceendlesselectricalpowerunless
theyaresuppliedwithfuelsandoxidants.
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30. Fuelcellconsistof
Twocatalyticelectrodes-Itmustbeagoodconductors,goodelectronsources,notbedeterioratedby
theelectrolyteheatandelectrodereactions,excellentcatalyst.Ex.Graphite,platinum,palladium,
silver,nickel.
Fuelandoxidant-Aresuppliedfromoutsidewhenrequired.Itisnotstoredinthecell.Frequentlyused
fuelsarehydrogen,methanol,ethanol,hydrazine,formaldehyde,carbonmonoxideandalkane.The
oxidantcouldbepureoxygen(or)air.
Electrolyte-Itisanion-conductingmaterialwhichseparatingthetwoelectrodes.Ex.AqeuousKOH(or)
H
2SO
4(or)ion-exchangeresin.
Attheanode,thefuelgetsoxidizedliberatingelectronsandtheoxidationproductsofthefuel.The
electronsliberatedfromtheanodereducetheoxidantatthecathode.Thus,theelectroncircuitor
currentdensityisestablished.
At anode: Fuel Oxidation product + ne
-
At cathode: Oxidant + ne
-
Reduction product
Overall cell reaction is Fuel + Oxidant Oxidation product + Electricity
Atypicalfuelcellcanberepresentedasfollows.
Fuel/Electrode//Electrolyte//Electrode/Oxidant
Components of Fuel Cells

31. 10-Jun-24
Becausefuelcellsgenerateelectricitythrough
chemistryratherthancombustion,theycan
achievemuchhigherefficienciesthantraditional
energyproductionmethodssuchassteam
turbinesandinternalcombustionengines.
Topushtheefficiencyevenhigher,afuelcell
canbecoupledwithacombinedheatand
powersystemthatusesthecell’swasteheatfor
heatingorcoolingapplications.

32. Classification
Hence based on the electrolyte used fuel
cells are classified as follows
Alkaline Fuel cells
Methanol –Oxygen Fuel cell
Phosphoric Acid Fuel Cells(PAFCs)
Molten Carbonate Fuel Cells(MCFCs)
Solid Oxide Fuel Cells(SOFC)
Solid Polymer Electrolyte Fuel
Cells(SPEFCS)
Microbial Fuel cells(MFCs)
10-Jun-24
Classification of fuel cell is very difficult as several
operational variable exists

33. Alkaline fuel cell (AFC)
Low temperature fuel cells (80°C) are used.
Porous carbon charged with Mi/Pd acts as anode.
Porous carbon charged with Ag-catalyst acts as cathode.
Hydrogen gas is fuel at anode.
Oxygen gas is fuel at cathode.
Aqueous KOH solution is used as electrolyte
Phosphoric acid fuel cell (PAFC)
Porous C + SiC + Teflon charged with Pt-catalyst acts as anode.
Porous C + SiC + Teflon charged with Ag-catalyst acts cathode.
Pure H
2gas is anodic fuel.
Pure O
2gas is cathodic fuel.
Concentrated phosphoric acid is used as electrolyte.
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34. Molten carbonate fuel cell (MCFC)
Anode is porous Ni/Ni –Cr alloy.
Cathode is porous NiO.
H
2gas or CO gas is fuel at anode
O
2 gas is fuel at cathode and it operates between 600 to 650°C.
Fused carbonate (eutectic mixture of 32% Li
2CO
3+ 48% NiAlCO
3+
K
2CO
3) in porous inorganic material is used as electrolytic.
Polymer electrolyte fuel cell (DMFC)
Two different porous gas diffused carbon electrodes charged with
platinum acts as both anode and cathode.
Methanol is used as anode fuel.
O
2gas is used as cathode fuel which is stable at 20°C to 90°C.
Nafion membrane with 50% water as electrolyte is used as electrolyte.
(Nafion, i.e., per fluorinated cation exchange polymer membrane)
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35. Alkaline Fuel Cells
Inalkalinefuelcells,theelectrolyteusedisanalkali,suchaspotassiumhydroxide(30–
40%aqueoussolution).
Thealkalinefuelcellsmakeuseofhighpurityhydrogenasfuelandoxygenasoxidant.
Thiskindoffuelcellisotherwiseknownashydrogen–oxygenfuelcell.
Thesearelowtemperature(80°C)fuelcells
Thistypeoffuelcellisbeingdevelopedfortransportapplicationsaswellasfor
stationaryfuelcellapplicationsandportablefuelcellapplications.
AFC’sarealsocalledBaconfuelcellsaftertheirBritishinventorFrancisThomas
Bacon.
10-Jun-24

36. Working :
An AFC uses two porous gas diffusion electrodes coated with
non precious metals as catalyst with KOH as electrolyte.
H
2as fuel is supplied at anode and O
2is supplied at cathode
At anode: H
2oxidizes to H
+
ions which react with OH
-
ions of
electrolyte to form H
2O.
The negatively charged e
-
cannot flow through electrolyte and
hence they must flow through external circuit forming electric
current.
O
2enter the fuel cell at cathode and picks up the e
-
and then travel
through the electrolyte towards the anode and combines with H
+
to form water.
AFC consumes pure H
2 and
O
2to produce portable
water, heat and electricity.

37. Advantages
Itissimple,lighterandcompactduetotheirthinsheetofpolymerelectrolyte.
It operates at lowtemperature.
Their reactionstarts quickly.
Itoperates at anyorientation.
It just emits water vapourand no other harmful chemicals to the environment.
The efficiency is higher than about 75 %.
It can replaces the use of batteries and causes less noise pollution.
Low maintenance cost
10-Jun-24

38. Disadvantages
ItisverysensitivetoCOandsulphurpoisoning sine hydrogen is obtained from the fossil fuels
through reforming.
Even trace amount of CO
2in fuel/air affect cell’s operation by converting KOH electrolyte
into potassium carbonate (solid) that blocks pores in the electrode and also reduce the
conductivity of fuel cell.
CO
2+ 2KOH K
2CO
3+ H
2O
ItrequirespureH
2gaswhichisdifficulttostore.
Itisverysensitivetolowhumidity.
Itneedshighcostplatinumascatalystforitsfunctioning,whichmakesthecellcostreally
expensive.
10-Jun-24

39. Applications
•AFC’s are limited to closed environments, such as space, undersea vechiclesand must
run on pure H2 and O2.
•Along with Phosphoric acid fuel cells, they were one of the earliest fuel cells
developed and used by NASA.
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40. MOLTENCARBONATE FUELCELLS(MCFCS)
10-Jun-24

41. MOLTENCARBONATE FUELCELLS(MCFCS)
It is a second generation fuel cells.
The molten carbonate fuel cell operates at approximately 650°C (1200°F).
The high operating temperature is needed to achieve sufficient conductivity of the
carbonate electrolyte.
A benefit associated with this high temperature is that noble metal catalysts are not
required for the cell processing.
Moltenlithium-potassiumcarbonatesaltsaretheelectrolytes.
H
2(or)COisthefuel,whileO
2istheoxidant.
Ashightemperatureisemployed,fairlylessexpensivecatalystslikeNi(or)NiO
areused.
TheanodecomprisesporousNiwith1-2%chromiumandthecathodecomprises
Niwith1-2%lithium.
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42. 10-Jun-24

43. Attheanode,hydrogenreactswiththecarbonateions(CO
3
2-
)toproduce
water,carbondioxide,andelectrons.
At the anode:
H
2+ CO
3
2–
→ H
2O + CO
2+ 2e
-
Theelectronstravelthroughanexternalcircuit,creatingelectricityandreturn
tothecathode.
There,oxygenfromtheairandcarbondioxiderecycledfromtheanodereact
withtheelectronstoformCO
3
2-
ionsthatreplenishtheelectrolyteandtransfer
currentthroughthefuelcell,completingthecircuit.
At the cathode:
½O
2+ CO
2+ 2e
–
→ CO
3
2-
The overall cell reaction
H
2+ ½O
2+ CO
2→ H
2O + CO
2
The emf generated is around 0.9 V.
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44. 10-Jun-24
Advantages
Molten carbonate fuel cells can convert the fuel into electricity almost 60 %. When the waste heat is
captured and used, overall fuel efficiencies can be increased upto85 %.
Because they do not contain platinum catalysts they are not susceptible to carbon monoxide or carbon
dioxide poisoning.
In fact, they can use carbon dioxide as fuel. This fact makes them very attractive for energy production in
countries like the United States that have large natural reserves of coal.

45. Disadvantages
Hightemperaturesdecreasecelllife.Thereiscurrentlyresearchunderwaytofindcorrosion
resistantmaterialsforuseathightemperatures.
Susceptibilitytopoisoningbysulfur,whichisfoundathighconcentrationinmanytypesofcoal.
Application
Thiscellisusedinchloroalkaliindustries
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46. DIRECTMETHANOLFUELCELL(DMFC)
Thedirectmethanolfuelcell(DMFC)utilizesmethanolasafuel.
mainadvantageistheeaseoftransportofmethanol,anenergy-denseyetreasonablystableliquidatall
environmentalconditions.
Inthisprocess,DMFCprovidescurrentbyelectrochemicallyoxidizingthemethanolattheanodeto
produceelectronswhichtravelthroughtheexternalcircuittothecathodewheretheyareconsumed
togetherwithoxygeninareductionreaction.
Thecircuitismaintainedwithinthecellbytheconductionofprotonsintheelectrolyte.
At anode: CH
3OH + H
2O → CO
2+ 6H
+
+ 6e
–
At cathode: 6H
+
+ 3/2 O
2+ 6e
–
→ 3H
2O
The overall cell reaction is:
CH
3OH + 3/2 O
2→ CO
2+ 2H
2O
In modern cells, the electrolytes based on proton conducting polymer electrolyte membranes (e.g., Nafion)
are often used, since they are convenient for cell design to withstand high temperature and pressure
operation. Cell emf is 1.2 V.
The overall reaction occurring in the DMFC is the same as that for the direct combustion of methanol.
10-Jun-24

47. Advantages
Itissuitableforportableelectronicsystemsof
lowpower,whichrunsforalongperiod.
Thefuelcelloperatesisothermallyandallthe
freeenergyassociatedwiththisreactionis
convertedintoelectricalenergy.
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Directmethanolfuelcell
Applications
MilitaryapplicationsofDMFCsareanemerging
applicationsincetheyhavelownoiseandthermal
signaturesandnotoxiceffluent.Theseapplications
includepowerforman-portabletacticalequipment,
batterychargers,andautonomouspowerfortestand
traininginstrumentation.

48. Types of Fuel Cells
Fuel Cell Operating Conditions
Alkaline FC (AFC) Operates at room temp. to 80
0
C
Apollo fuel cell
Proton Exchange
Membrane FC (PEMFC)
Operates best at 60-90
0
C
Hydrogen fuel
Originally developed by GE for space
Phosphoric Acid FC (PAFC)Operates best at ~200
0
C
Hydrogen fuel
Stationary energy storage device
Molten Carbonate FC
(MCFC)
Operates best at 550
0
C
Nickel catalysts, ceramic separator membrane
Hydrocarbon fuels reformed in situ
Direct Methanol Fuel Cell
(DMFC)
Operates best at 60-90
0
C
Methanol Fuel
For portable electronic devices

49. ADVANTAGES OFFUELCELLS
Fuelcellshaveahighefficiencyofenergy
conversion(75to83%),i.e.,chemicalenergyto
electricalenergy.
Fuelcellsmakeuseofhydrocarbongasfromfossil
fuelandtheresultantemissionsofpollutantsare
withinthepermissiblelimits.
Fuelcellhavelowmaintenancecost.
Fuelcellshavequickstartsystem.
Theregenerativehydrogen-oxygenfuelcell
systemshavegreatapplicationsinspaceresearch.
Theyalsoproducepotablewaterasendproduct.
Infuelcell,lowcostfuelscanbeusedprovidedit
shouldbeoperatedathighertemperatures
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50. Fuel Cells in India
Ahydrogenfuelcellbuswaslaunchedin2019inIndia
byTataMotorsincollaborationwiththeIndianSpace
ResearchOrganization(ISRO)andIndianOil
(IOCL).Inaddition,Hyundaialsoseekstoplaceitsfirst
fuelcellNEXOSUVinIndiaby2021,andplanson
buildingtherequiredhydrogeninfrastructuretosupport
thevehiclesnearDelhi.
10-Jun-24
Tata Starbus Fuel Cell, the first hydrogen
fuel cell powered bus in India.
PrimeMinisterNarendraModilaudedasahugeresolutionthe
‘HydrogenMission’announcedintheBudget2021,underliningthat
futurefuelsandgreenenergyarethewayforwardforattainingself-
sufficiencyforIndia’senergyrequirements.India’sveryfirsthydrogen
fuelcellpassengervehiclewastestedinOctoberlastyearbyCSIR
(CouncilofScientificandIndustrialResearch)andKPITTechnologies.
CSIRandKPIThavedevelopeda10kWe(Kilowatt-electric)
automotivegradeLT-PEMFC(low-temperaturePEMfuelcell)