Batteries Chemistry Notes

Batteries Chemistry Notes

Batteries :

→ When more than one calls are attached in series then battery is obtained. In fact, battery is an arrangement of Galvanic cells in series. Battery converts chemical energy of redox reaction into electric energy. There are of two types of batteries:

→ Primary Batteries – In primary batteries, reaction takes place only once and battery becomes inactive after some time and can not be reused again. These are of following types:

→ Dry Cell – It was discovered by Leclanche. So, it is called Leclanche cell. It is used generally in transistors and watches. This cell contains a zinc pot which acts as anode and the rod of carbon graphite, which is surrounded by powdered manganese dioxide and carbon, acts as cathode. The place between electrodes is filled with moist paste of ammonium chloride (NH4 Cl) and zinc chloride (ZnCl2). In this cell, electrode reactions are complex but these can be written simply as follows:

Batteries Chemistry Notes 1

Batteries Chemistry Notes 2

→ In cathode reaction, manganese is reduced from +4 to +3 oxidation state. Ammonia produced in the reaction forms a complex [Zn(NH3)4]2+ with Zn2+ ion. The cell potential is approximate 1.5 V The age of dry cell is not so high; since NH4Cl corrodes zinc apparatus due to acidic nature when the cell is not used.

→ Mercury Cell – Mercury cell is used in hearing devices, watches etc. which require less amount of electricity. In this cell, zinc-mercury amalgam acts as anode and HgO and paste of carbon acts as cathode. The paste of KOH and ZnO is electrolyte. The electrode reaction of cell is given below:

Batteries Chemistry Notes 3

  • Anode : Zn(Hg) + 2OH → ZnO(s) + H2O + 2e
  • Cathode : HgO + H2O + 2e → Hg(l) + 2OH

Complete cell reaction is represented as follows:

Zn(Hg) + HgO(s) → ZnO(s) + 2Hg(l)

→ Cell potential is approximate 1.35 V and constant in complete working, because no such ion is present in complet cell reaction whose cell potential can be changed in complete working of cell due to concentration present in solution.

Batteries Chemistry Notes

→ Secondary or Storage Batteries – These are reversible Galvanic cells. In these batteries, the substances having high energy produce electric current on rapid reaction and become inactive. These substances made active again by external sources and those substances are used again in cell. So, these cells can be recharged again. Storage battery can be discharged and charged many times. Main examples of these batteries are as follow:

→ Lead Storage Cell – In this cell, anode is made up of lead and cathode is lead grid filled with PbO2.
It contains 38% H2SO4 as electrolyte.

Following reactions take place in it:

Batteries Chemistry Notes 4

So, net reaction of cathode and anode is given below:

Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l) The reaction is reversible on charging of battery and anode and cathode change in PbSO4(s)). Pb and PbO2 respectively.

Reversed reaction :

2PbSO4(s) + 2H2O(l) →Pb(2) + PbO2 + 2H2SO4(aq)

Nickel Cadmium Storage Cell-It is an important storage cell whose working period is more than lead storage battery but its costing is more. Its discharge reaction is given below:

Batteries Chemistry Notes 5

Batteries Chemistry Notes 6

Difference between Primary and Secondary Cell :

Primary Cell Secondary Cell
Primary cells are irreversible. Secondary cells are reversible.
Chemical reaction takes place only in one direction. Chemical reaction takes p1ace in both directions.
These types of cells can not be charged. These types of cells can be charged.

Chemistry Notes