What is Electric Battery ?

This is one way of describing how electrical potential causes electrons to flow through the circuit.

However, these electrochemical processes change the chemicals in anode and cathode to make them stop supplying electrons. So there is a limited amount of power available in a battery.

When you recharge a battery, you change the direction of the flow of electrons using another power source, such as solar panels.

The electrochemical processes happen in reverse, and the anode and cathode are restored to their original state and can again provide full power.

Batteries are a collection of one or more cells whose chemical reactions create a flow of electrons in a circuit. All batteries are made up of three basic components: an anode (the ‘-’ side), a cathode (the ‘+’ side), and some kind of electrolyte (a substance that chemically reacts with the anode and cathode).

When the anode and cathode of a battery is connected to a circuit, a chemical reaction takes place between the anode and the electrolyte.

This reaction causes electrons to flow through the circuit and back into the cathode where another chemical reaction takes place.

When the material in the cathode or anode is consumed or no longer able to be used in the reaction, the battery is unable to produce electricity.

Batteries that must be thrown away after use are known as primary batteries. Batteries that can be recharged are called secondary batteries.

Without batteries, your quadcopter would have to be tethered to the wall, you would have to hand crank your car, and your Xbox controller would have to plugged in all the time (like in the good old days). Batteries offer a way to store electrical potential energy in a portable container.

One fateful day in 1780, Italian physicist, physician, biologist, and philosopher, Luigi Galvani, was dissecting a frog attached to a brass hook.

As he touched the frog’s leg with an iron scapel, the leg twitched. Galvani theorized that the energy came from the leg itself, but his fellow scientist, Alessandro Volta, believed otherwise.

Volta hypothesized that the frog’s leg impulses were actually caused by different metals soaked in a liquid.

He repeated the experiment using cloth soaked in brine instead of a frog corpse, which resulted in a similar voltage.

Volta published his findings in 1791 and later created the first battery, the voltaic pile, in 1800.

Volta’s pile was plagued by two major issues: the weight of the stack caused the electrolyte to leak out of the cloth, and the particular chemical properties of the components resulted in a very short life span (about an hour).

The next two hundred years would be spent perfecting Volta’s design and solving these issues.

The second problem, short life span, was caused by the degradation of the zinc due to impurities and a build up of hydrogen bubbles on the copper.

In 1835, William Sturgeon discovered that treating the zinc with mercury would prevent degradation.

In 1835, William Sturgeon discovered that treating the zinc with mercury would prevent degradation.

The British chemist John Frederic Daniell used a second electrolyte that reacted with the hydrogen, preventing buildup on the copper cathode. Daniell’s two-electrolyte battery, known as the “Daniell cell,” would become a very popular solution to providing power to the budding telegraph networks.

In 1859, the French physicist Gaston Planté created a battery using two rolled sheets of lead submerged in sulfuric acid. By reversing the electrical current through the battery, the chemistry would return to its original state, thus creating the first rechargeable battery.

Later, in 1881, Camille Alphonse Faure improved Planté’s design by forming the lead sheets into plates.

This new design made the batteries easier to manufacture, and the lead acid battery saw wide-spread use in automobiles.

Up until the late 1800s, the electrolyte in batteries was in a liquid state.