Comparative Study of Battery Technology Assignment Sample

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COMPARATIVE STUDY OF BATTERY

TECHNOLOGY

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Table of Contents INTRODUCTION .......................................................................................................................... 1

TASK1. ........................................................................................................................................... 1

TASK2. ........................................................................................................................................... 3

CONCLUSION ............................................................................................................................... 6

REFERENCES ............................................................................................................................... 6



Table of Figures

Table 1: Comparison and contrast between battery technologies ................................................... 4


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INTRODUCTION

The prevailing energy crisis has raised the awareness for the utility of battery technology.

Batteries, in which electricity is stored in chemical form can be recharged and reused as a source

of power (Batteries included?, 2013). Battery technology can be used for clearing and

accelerating the path to a more energy dependent and greener framework. In the present report, a

general overview of the battery cell has been provided. The report discusses the method which

helps in the conversion of chemical energy into electrical energy. Differentiation has been made

between the primary and secondary cell types. An attempt has been made to compare and

contrast carbon-zinc, lead-acid and alkaline batteries.

TASK1.

A device that consists of one or more electrochemical cells used for converting stored

chemical energy into electrical energy is known as a battery. Generally, each battery cell consists

of three parts. They are the following:

Cathode- This is the positive terminal. It is the oxidizing electrode. The electrons are

acquired by this electrode form the external circuit (Kiehne, 2003). As a result, it is

reduced during the electrochemical reaction.

Anode- This is the negative terminal. Anode works as a reducing electrode. Electrons are

released from it to the external circuit. During an electrochemical reaction, it gets

oxidized.




Electrolyte- This is the third component of a battery cell is the electrolyte. This provides

the medium for facilitating the mechanism of ion transport between the cathode and the

anode of the cell (Pavlov, 2011). Generally, electrolytes are in the form of liquids such as

water and other solvents. These consist of dissolved salts, acids and alkalis that are

required for the conduction of the ions. However, in some batteries including the

conventional batteries, the electrolyte can be in solid form that acts as ionic conductor at

room temperature.

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Hence, an excess of positive ions are produced at the cathode. These positive ions are

actually atoms that lack electrons and thus carry a positive charge. In a battery, two dissimilar

metals are connected to each other through the use of a conducting medium or electrolyte (Alotto

and et.al., 2013). As a result of this, electrons develop a tendency to pass from the metal that has

smaller affinity for electrons to the metal that has a greater affinity for electrons. Thus, metal

with smaller affinity for electrons becomes positively charged while the other with greater




affinity becomes negatively charged. Hence, there develops a potential difference

between the metals until it is balanced with the tendency of electron transfer between the metals.

Hence, in a battery, both oxidation and reduction reactions occur simultaneously. This is known

as redox reaction. The ions are allowed by the electrolytes to move between the electrodes and

terminals. As such, the current is permitted to flow out of the battery for performing work.

A battery is a collection of two or more primary or secondary battery cells which convert

chemical energy into electrical energy. A primary call is a battery which can only be used once

and discarded. It cannot be recharged with electricity. Current is produced by these cells

immediately on assembly. These cells cannot be recharged as chemical reactions cannot be

reversed and the active materials are not in a position to return to the original form. When a

primary cell is used, the chemicals in the battery are used up by the chemical reaction for

producing power (Dijkhuizen and et.al., 2012). When the chemicals are used up, the battery

stops producing electricity and becomes useless. Secondary cells are those in which the

electrochemical reaction is reversible. Reconstitution of the original chemical compounds can be

done with the application of an electrical potential between the electrodes. Hence, these cells can

be discharged and recharged many times.

TASK2.

Comparison and contrast of three battery technologies has been done in the following manner:

Zinc-carbon battery technology- This is type of primary battery. It is the most common form of a

dry cell. It is based on the principle in which paste electrolyte is used with only enough moisture

that allows the current to flow. In this, the battery is packed in a zinc can. This can serves the




purpose of a container as well as provides a negative terminal for the cell (Southee, 2007). A

carbon rod that is surrounded by a mixture of manganese dioxide and carbon powder acts as the

positive terminal. As electrolyte, a paste of zinc chloride and ammonium chloride dissolved in

water is sued. These batteries are least expensive batteries. This battery technology allows the

cell to be used and operated in any orientation without the risk of spilling. This is because of

absence of free liquid.



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Table 1: Comparison and contrast between battery technologies

Type Chemistry Sizes and common

applications

Features

Zinc-carbon Zinc alloy as anode

Manganese dioxide

as cathode

1.55 volts per cell

Cylindrical and

rectangular jackets.

Used in remote

controls, flashlights

etc.

Cheap and light

weight

Low energy density

Poor performance at

low temperatures

Lead-acid Lead as anode

Lead dioxide as

cathode

Sulphuric acid as

electrolyte

Wide range of sizes

Used in

automobiles, boats

etc.

Cheapest and

heaviest battery

Long life

Alkaline Reaction between

manganese dioxide

and zinc

Alkaline electrolyte

of potassium

hydroxide

Cylindrical jackets

Used in power

tools, bio medical

equipment, smoke

alarms etc.

Higher energy

density

Longer shelf life






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REFERENCES

Journals and books

Alotto, P., and et.al., 2013. Large scale energy storage with redox flow batteries. COMPEL: The International Journal for Computation and Mathematics in Electrical and Electronic Engineering. 32(5). pp.1459 – 1470.

Bogue, R., 2010. Powering tomorrow's sensor: a review of technologies – Part 1. Sensor Review. 30(3). pp.182 – 186.

Bogue, R., 2010. Wireless sensors: a review of technologies, products and applications. Sensor Review. 30(4). pp.285 – 289.

Dijkhuizen, F., and et.al., 2012. Dynamic energy storage for smart grids. COMPEL: The International Journal for Computation and Mathematics in Electrical and Electronic Engineering. 31(1). pp.279 – 293.

Kiehne, A. H., 2003. Battery Technology Handbook. 2 nd ed. CRC Press.

Malone, E., Berry, E., and Lipson, H., 2008. Freeform fabrication and characterization of Zn-air batteries. Rapid Prototyping Journal. 14(3). pp.128 – 140.

Pavlov, D., 2011. Lead-Acid Batteries: Science and Technology: Science and Technology. Elsevier.

Southee, D., 2007. Lithographically printed voltaic cells – a feasibility study. Circuit World. 33(1). pp.31 – 35.

Online

Batteries included?. 2013. [Online]. Available Through: <http://www.economist.com/news/science-and-technology/21571117-search-better-ways-storing-electricity-hotting-up-batteries>. [Accessed on 10 January 2013].


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