Primary and secondary batteries | NCERT electrochemistry JEE / NEET / Boards

Primary and secondary batteries | NCERT electrochemistry JEE / NEET / Boards
What is a Battery?
A Battery is a device consisting of one or more electrical cells that convert chemical energy into electrical energy. Every battery is basically a galvanic cell where redox reactions take place between two electrodes which act as the source of the chemical energy.
Battery types
Batteries can be broadly divided into two major types.
Primary Cell / Primary battery
Secondary Cell / Secondary battery
Based on the application of the battery, they can be classified again. They are:
Household Batteries
These are the types of batteries which are more likely to be known to the common man. They find uses in a wide range of household appliances (such as torches, clocks, and cameras). These batteries can be further classified into two subcategories:
Rechargeable batteries Nickel
Examples: Cadmium batteries, Lithium-Ion
Non-rechargeable batteries
Examples: Silver oxide, Alkaline & carbon zinc
Industrial Batteries
These batteries are built to serve heavy-duty requirements. Some of their applications include railroad, backup power and more for big companies. Some examples are:
Nickel Iron
Wet Nickel Cadmium (NiCd)
Vehicle Batteries
These are more user-friendly and a less complicated version of the industrial batteries. They are specifically designed to power cars, motorcycles, boats & other vehicles. An important example of a vehicle battery is the Lead-acid battery.
Battery or cells are referred to as the parallel combination of electrochemical cells. The major difference between a primary cell and the secondary cell is that primary cells are the ones that cannot be charged but secondary cells are the ones that are rechargeable.
Primary cell
Primary cells have high density and get discharged slowly. Since there is no fluid inside these cells they are also known as dry cells. The internal resistance is high and the chemical reaction is irreversible. Its initial cost is cheap and also primary cells are easy to use.
Secondary cell
Secondary cells have low energy density and are made of molten salts and wet cells. The internal resistance is low and the chemical reaction is reversible. Its initial cost is high and is a little complicated to use when compared to the primary cell.
Difference Between Primary Cell and Secondary Cell
Primary cells are the ones which cannot be recharged and have to be discarded after the expiration of the lifetime whereas, secondary cells need to be recharged when the charge gets over. Both the types of battery are used extensively in various appliances and these cells differ in size and material used in them.
Frequently Asked Questions - FAQs
Q1 Give e some examples of secondary cells.
Lithium-ion battery and nickel-cadmium.
Q2 Give some examples of primary cells.
Alkaline batteries and dry cells are examples of primary cells.
Q3 What is the Function of a Salt Bridge in an Electrochemical Cell?
The salt bridge completes the circuit of an electrochemical cell, thereby allowing the flow of current through it. It also helps to maintain the overall electrical neutrality of the cell.
Q4. What is Standard Electrode Potential?
The standard electrode potential of an electrode can be defined as the potential difference that arises between the electrode and the electrolyte under standard conditions (Temperature = 298K, pressure = 1 atm, unity concentration of reacting species).
Q5 What are the Key Differences between Cathode and Anode?
The cathode of an electrochemical cell is the site at which reduction occurs. It is generally represented by a positive (+) sign. The electrons flow from the anode towards the cathode. In electrochemical cells, the anode is the electrode at which oxidation occurs. It is denoted by a negative (-) sign.
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