Презентация на тему Primary batteries

small-scale source of electrical energy.
Has changed very little in

the last 100 years.
An electrolyte composed of a moist paste of zinc chloride and ammonium chloride plays the same role as the salt bridge.

This battery was invented by Goerge Lionel Leclanche in 1866

the zinc case produces electrons:
Zn(s) → Zn2+(aq) + 2e-
At

the cathode (+) Manganese dioxide is reduced in a complicated reaction that is thought to be:
2MnO2(s) + 2NH4+(aq) + 2e- → Mn2O3(s) + 2NH3(aq) + H2O(l)

1.5 volts, but this diminishes significantly during use.
To maintain

a net forward reaction, the soluble reaction products must migrate away from the electrodes.
During use the build up of products around the electrodes slows and can even stop the forward reaction.
This is known as polarisation. If the cell is allowed to rest, the products migrate away from the electrodes and the cell can recover.

of a zinc carbon battery is determined by type

of anode and cathode materials used in the battery cell. In zinc carbon battery cell, zinc is anode material and manganese dioxide is cathode material. Electrode potential of zinc is – 0.7 volt whereas electrode potential of manganese dioxide is 1.28.

Therefore, theoretical voltage of each cell should be – ( - 0.76) + 1.23 = 1.99 V but considering many practical conditions, the actual voltage output of a standard zinc carbon battery is not more than 1.5 V.

Leclanche’ Battery
The cost of this battery cell is quite

low.
Various shapes, sizes and capacities of these cells are easily available.
Long traditional reliability.


Disadvantages of Leclanche’ Battery
Its energy density is quite low.
It gives poor service in low temperature.
It has poor leakage resistance.
Cannot perform efficiently at high current drain application.
Self life is not very good.
Its voltage falls steadily with discharge.

being a collection of multiple cells) are a type

of disposable battery or rechargeable battery dependent upon the reaction between zinc and manganese(IV) oxide (Zn/MnO2).
Alkaline battery is an improved dry cell.
The alkaline battery gets its name because it has an alkaline electrolyte of potassium hydroxide, as opposed to the acidic electrolyte of the zinc-carbon batteries
Zinc in a powdered form increases the surface area of the anode, allowing more particle interaction. This lowers the internal resistance and increases the power density

steel can, which is the cathode current collector.
The

cathode mixture is a compressed paste of manganese dioxide with carbon powder added for increased conductivity.
The hollow center of the cathode is lined with a separator, which prevents mixing of the anode and cathode materials and short-circuiting of the cell.
The separator is made of a non-woven layer of cellulose or a synthetic polymer. The separator must conduct ions and remain stable in the highly alkaline electrolyte solution.
The anode is composed of a dispersion of zinc powder in a gel containing the potassium hydroxide electrolyte. To prevent gassing of the cell at the end of its life, more manganese dioxide is used than required to react with all the zinc.

powder
Electrolyte : Potassium hydroxide(KOH)

Zn (s) + 2OH− (aq) →

ZnO(s) + H2O (l) + 2e−
Cathode(Reduction) :
2MnO2 (s) + H2O (l) + 2e− →Mn2O3 (s) + 2OH− (aq)
The overall reaction is:
Zn + 2MnO2 —> ZnO + Mn2O3 ;E=1.5 V

to function in sub-zero temperatures.
Less leakage than Leclanché

cells
Available in a wide range of sizes including AAA, AA, C, D and 9Volt sizes.
Suitable for a wide range of consumer applications
Made from non toxic chemicals
No voltage drop and longer shell life than dry cell because of alkaline electrolyte