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Types of Batteries: Primary & Secondary Cells Explained
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You may find them as MCQs, short answers, or even diagram questions. French engineer Georges Leclanché’s prototype of the zinc–manganese dioxide system paved the way for the development of the modern primary battery. The original version of the Leclanché cell was “wet,” as it had an electrolyte consisting of a solution of ammonium chloride. The idea of employing an immobilized electrolyte was finally introduced in the late 1880s and launched the dry-cell industry that continues to flourish today. In 1859 Gaston Planté of France invented a lead-acid cell, the first practical storage battery and the forerunner of the modern automobile battery. Planté’s device was able to produce a remarkably large current, but it remained a laboratory curiosity for nearly two decades.
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Tried, tested, and trusted, lead-acid batteries have been with us since the middle of the 19th century. With an overall rating of 12 volts, they have six separate cells, each producing 2 volts. Crudely reduced to its basic components, each cell has a “spongy” lead metal electrode (negative), a lead dioxide electrode (positive), and a sulfuric acid electrolyte. At school, you may have learned that the cathode is the negative electrode and the anode the positive electrode? However, that really applies only to things like electrolysis (passing electricity through a chemical to split it up). Batteries are like electrolysis going backwards (they split up chemicals to make electricity) so the terms anode and cathode are switched around.
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Battery performance is thus limited by the diffusion rates of internal chemicals as well as by capacity. Primary batteries are single-use and cannot be recharged (alkaline, zinc-carbon). Secondary batteries are rechargeable and can be used hundreds of times (lithium-ion, NiMH, lead-acid).
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However, a solar charger might be a better option if AC power is unavailable where you store your equipment. Many vehicles now come with key fobs always searching for a key, Bluetooth, Wi-Fi, GPS, and whatever the next great device is, I’m sure it will be installed in a vehicle. All these electronics require a reliable power source, and poor battery conditions can wreak havoc on electrical systems.
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Secondary Batteries
We recommend buying a new Dell laptop battery when the run time does not meet your needs. Yes, there are third-party tools available, but the built-in Windows battery report is usually sufficient for most users. However, third-party tools can offer additional features and insights. After completing these steps, you’ll have a comprehensive understanding of your battery’s condition.
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However, for batteries where the state of charge is low, direct recycling may not be worth the investment. On the macrostructral level (length scale 0.1–5 mm) almost all commercial lithium-ion batteries comprise foil current collectors (aluminium for cathode and copper for anode). Copper is selected for the anode, because lithium does not alloy with it. Aluminum is used for the cathode, because it passivates in LiPF6 electrolytes.
Over the course of several charge and discharge cycles, the shape of the battery’s crystals becomes less ordered. This is exacerbated when a battery is discharged/recharged at a high rate—for example, if you drive your electric car in big bursts of speed rather than steadily. High-rate cycling leads to the crystal structure becoming more disordered, with a less efficient battery as a result. So the cell generally has some sort of barrier to prevent this from happening.
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Such batteries produce hydrogen, which is very explosive, when they are overcharged (because of electrolysis of the water in the electrolyte). During normal use, the amount of overcharging is usually very small and generates little hydrogen, which dissipates quickly. The C-rate is a measure of the rate at which a battery is being charged or discharged.
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To avoid confusion, I suggest it’s best not to use the terms anode and cathode at all. When you connect a battery’s two electrodes into a circuit (for example, when you put one in a flashlight), the electrolyte starts buzzing with activity. Slowly, the chemicals inside it are converted into other substances. Ions (atoms with too few or too many electrons) are formed from the materials in the electrodes and take part in chemical reactions with the electrolyte. At the same time, electrons march from one terminal to the other through the outer circuit, powering whatever the battery is connected to.
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