This document summarizes different types of batteries - primary batteries, secondary batteries, and fuel cells. It describes that primary batteries have an irreversible chemical reaction and cannot be recharged, secondary batteries have a reversible reaction and can be recharged, and fuel cells continuously convert chemical energy directly to electrical energy as long as fuel is supplied. Examples of each type are provided, including the dry cell/Leclanche cell, lithium-ion battery, and hydrogen-oxygen fuel cell. Their components, reactions, and applications are briefly outlined.

1. Batteries
Dr. B. Santosh Kumar
&
Dr.K.V.Nagalakshmi

2. Battery is an electrochemical cell or several
electrochemical cells connected in series to produce an
electric current.
An electrochemical cell is a device that can generate
electrical energy from the chemical reactions occurring in
it, or use the electrical energy supplied to it to facilitate
chemical reactions in it. These devices are capable of
converting chemical energy into electrical energy, or vice
versa.
A battery is a device that stores chemical energy and
converts it to electrical energy. Any galvanic cell could be
used as a battery.
Introduction

3. Batteries are mainly classified into 3 types.
Primary batteries
Secondary Batteries
Fuel cells
Classification

4. Primary batteries
In primary cells the cell reaction is not
reversible.
No electricity is produced after complete
conversion of the reactants to products and
the cell becomes dead.
These batteries are used as source of DC
power.
Examples:
Dry cell (Leclanche cell),

5. Secondary batteries
The cells in which the cell reaction is reversed by
passing direct current in opposite direction.
It can operate both as a voltaic cell and as an
electrolytic cell.
The secondary batteries can be used through a large
number of cycles of discharging and charging. They are
used as a source of DC power.
Examples:
Lead-acid battery
Li-ion battery

6. Fuel Cells
A fuel cell is a galvanic cell in which chemical energy
of a fuel – oxidant system is converted directly into
electrical energy in a continuous electrochemical
process.
The fuel and oxidants are continuously and
separately supplied to the electrodes of the cell where
they undergo reactions.
Fuel cells are capable of supplying current as long as
reactants are supplied.
Examples:
H2-O2 Fuel cell or Alkaline Fuel cell

7. S.No. Primary Cell Secondary Cells Fuel Cells
1
Cell reaction is
irreversible
Reversible Combustion
reaction of fuel
takes place.
2
Cannot be recharged Can be recharged Cannot be
recharged
3
Cannot be reused Can be reused Cannot be
reused
4
Can act as galvanic
cell
Act as both galvanic
cell as well electrolytic
cell
Act as only
galvanic cell
5
Cannot be used as
storage devices
Used as energy
storage devices
Do not store
energy
6
Relative short shelf-
life
Longer shelf-life As long as fuel is
supplied
7
Eg: Dry cell Eg: Lithium ion
battery
Eg: H2-O2 fuel
cell
Comparison

8. Advantages of fuel cell
1. High efficiency
2. Product is harmless and useful –H2O
3. Silent Operation

9. Primary batteries
Dry cell / Leclanche cell:
Anode: Zn-container
Cathode: Graphite rod
Electrolyte: Mixture of MnO2(s), NH4Cl (aq) and
ZnCl2(s) to which starch is added to make a
paste
Voltage: 1.5 V

10. Source:
https://opentextbc.ca/chemistry/chapter/17-5-
batteries-and-fuel-cells/

12. Advantages:
Low price;
gives voltage of about 1.5 V;
normally works without leaking (leak proof cells);
possess high energy density;
non- toxic;
contains no liquid electrolytes.
Applications: Dry cell is used in consumer electronic devices like
calculators, transistor radios, flash lights, quartz wall clocks,
walkman etc. and in small portable appliances where small
amount of current is needed.

13. Secondary Battery-Lithium Ion battery
Lithium ion Battery :
Anode: Lithiated intercalated Carbon
Cathode: Lithiated metal oxide
Electrolyte: Mixture of lithium salts (LiX)

17. Applications
• Power backups/UPS
• Mobile, Laptops, and other commonly used
consumer electronic goods
• Voltage-3.6 V

18. H2-O2 Fuel Cell (Alkaline fuel cell)
• Anode-Carbon/Pt
• Cathode-Carbon/Ag
• Electrolyte- KOH
• Fuel-H2
• Oxidant-O2
• Operating temperature-70oC

19. H2-O2 Fuel Cell (Alkaline fuel cell)

21. Applications
• Alkaline fuel cells consume hydrogen and pure
oxygen, to produce potable water, heat, and
electricity. They are among the most efficient
fuel cells, having the potential to reach 70%.
• NASA has used alkaline fuel cells since the
mid-1960s, in the Apollo-series missions and
on the Space Shuttle.