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ᴡʜᴀᴛ ɪꜱ ᴀ ʙᴀᴛᴛᴇʀʏ🔋

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ᴡʜᴀᴛ ɪꜱ ᴀ ʙᴀᴛᴛᴇʀʏ🔋

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► A battery is an electrochemical cell that can convert chemical energy to electricity generation due to a spontaneous oxidation-reduction or redox reaction that involves electron transfer from one substance to the other.

► The essential components of a battery are the anode, cathode, and electrolyte. The anode is the electrode at which the oxidation half-reaction occurs, and the cathode is the electrode at which the reduction half-reaction happens. The electrolyte is the solution that contains positive or negative charges that assist in regulating the chemical reaction.

► In connecting the battery to an electrical circuit, the anode and cathode will react to the electrolyte solution in a redox reaction until the battery output depletes as the electrodes dissolve, requiring it for replacement.

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ᴡʜᴀᴛ ɪꜱ ᴀ ꜰᴜᴇʟ ᴄᴇʟʟ🪫

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ᴡʜᴀᴛ ɪꜱ ᴀ ꜰᴜᴇʟ ᴄᴇʟʟ🪫

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► A fuel cell is an electrochemical cell that utilizes the chemical energy of fuels, such as hydrogen, and oxidizing agents, like oxygen, to produce electricity through a spontaneous redox reaction.

► The necessary components of a fuel cell are the anode, cathode, electrolyte exchange membrane, fuel, and air. The fuel will pass through the anode, where oxidation will occur. On the other hand, air will go through the cathode, which reduction occurs. The electrolyte exchange membrane conducts the ions to the cathode as the oxygen from the air combines with the fuel's hydrogen. Thus, its byproduct is water.

►  As the fuel cell have a constant supply of fuel and air to maintain its chemical reaction, it constantly creates electricity. With this, it serves as a renewable energy source, as its only byproduct is water.

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3 ꜱɪᴍɪʟᴀʀɪᴛɪᴇꜱ ʙᴇᴛᴡᴇᴇɴ ʙᴀᴛᴛᴇʀɪᴇꜱ & ꜰᴜᴇʟ ᴄᴇʟʟꜱ🤔

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3 ꜱɪᴍɪʟᴀʀɪᴛɪᴇꜱ ʙᴇᴛᴡᴇᴇɴ ʙᴀᴛᴛᴇʀɪᴇꜱ & ꜰᴜᴇʟ ᴄᴇʟʟꜱ🤔

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► Batteries and fuel cells are electrochemical cells that convert chemical energy to electrical energy.

► They utilized a spontaneous redox reaction involving electron transfer from one substance to another, producing an electric current.

► Both have anodes and cathodes that rely on an electric circuit to produce a current flow.

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3 ᴅɪꜰꜰᴇʀᴇɴᴄᴇꜱ ʙᴇᴛᴡᴇᴇɴ ʙᴀᴛᴛᴇʀɪᴇꜱ & ꜰᴜᴇʟ ᴄᴇʟʟꜱ🧐

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3 ᴅɪꜰꜰᴇʀᴇɴᴄᴇꜱ ʙᴇᴛᴡᴇᴇɴ ʙᴀᴛᴛᴇʀɪᴇꜱ & ꜰᴜᴇʟ ᴄᴇʟʟꜱ🧐

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► Batteries stores electrical energy from their stored chemical energy, while fuel cells require a source of fuel and air to produce an electrical charge.

► The chemical energy of batteries stems from ions of metals. The chemical energy of fuel cells comes from fuel and air.

► Batteries deplete their electrical output once the anode and cathode metal electrode dissolves, requiring the whole battery to be replaced. On the flip side, once a fuel cell completely used fuel and air, it can be renewable supplied again to continually produced electrical energy.

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ᴛʏᴘᴇꜱ ᴏꜰ ʙᴀᴛᴛᴇʀɪᴇꜱ⚡

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ᴛʏᴘᴇꜱ ᴏꜰ ʙᴀᴛᴛᴇʀɪᴇꜱ⚡

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Primary Batteries
↳ Primary batteries, also known as disposable batteries utilize the electrical energy from the chemical energy of the decomposition of the electrode and electrolyte, resulting in an irreversible chemical process of the breakdown of electrodes or electrolyte. Thus, it requires replacing the battery.
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Secondary Batteries
↳A secondary battery is an electrochemical cell that has reversible cell reactions. It means that the chemical reaction within the battery is restorable by passing a current flow into it. Thus, it is rechargeable from an external electrical source.

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ɪꜱ ᴀ ꜰᴜᴇʟ ᴄᴇʟʟ ᴀ ᴘʀɪᴍᴀʀʏ ᴏʀ ꜱᴇᴄᴏɴᴅᴀʀʏ ʙᴀᴛᴛᴇʀʏ?

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ɪꜱ ᴀ ꜰᴜᴇʟ ᴄᴇʟʟ ᴀ ᴘʀɪᴍᴀʀʏ ᴏʀ ꜱᴇᴄᴏɴᴅᴀʀʏ ʙᴀᴛᴛᴇʀʏ?

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Fuel cells are considered a type of primary cell as they are not rechargeable through an external electrical source. However, they are distinct as they never deplete as long as there is a constant source of fuel and air that continues the chemical reaction within the cell.

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ᴇxᴀᴍᴘʟᴇ ᴏꜰ ᴘʀɪᴍᴀʀʏ ʙᴀᴛᴛᴇʀɪᴇꜱ🔋

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ᴇxᴀᴍᴘʟᴇ ᴏꜰ ᴘʀɪᴍᴀʀʏ ʙᴀᴛᴛᴇʀɪᴇꜱ🔋

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Carbon Zinc Heavy Duty Cell (Zinc-Acidic Manganese Dioxide Battery)
► Lowest-cost primary cell
► Low power, but a good shelf life
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Alkaline Cell (Zinc-Alkaline Manganese Dioxide Battery)
► The most commonly used primary cell
► More power per use that Carbon-zinc and secondary batteries and excellent shelf life
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Lithium Cells
► Offer performance advantages beyond the capabilities of a conventional aqueous electrolyte battery system.
► Shelf life above ten years
► Works in low temperatures
► Commonly used in small formats, such as coin cells
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Silver Oxide Cells
► High energy density
► Expensive
► Mainly used in button cell batteries
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Zinc Air Cells
► Long run time
► The anode is inside the cell, and the cathode is the ► oxygen from atmospheric air.

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ᴇxᴀᴍᴘʟᴇ ᴏꜰ ꜱᴇᴄᴏɴᴅᴀʀʏ ʙᴀᴛᴛᴇʀɪᴇꜱ🪫

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ᴇxᴀᴍᴘʟᴇ ᴏꜰ ꜱᴇᴄᴏɴᴅᴀʀʏ ʙᴀᴛᴛᴇʀɪᴇꜱ🪫

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Rechargeable Alkaline Batteries
► Lowest-cost rechargeable cells
► Long shelf life
► Useful to moderate power application
► Lesser cycle than most secondary batteries
► Great consumer's choice with the benefits of alkaline cells with the added benefit of recharging
► No toxic ingredients
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Nickel Cadmium Batteries
► Rugged and reliable
► High power capability
► Wide operating temperature range
► Long cycle life
► Low run time per charge
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Nickel-Metal Hydride
► Extension of the old fashioned Nickel-Cadium batteries
► Same voltage as Nickel-Cadium batteries but offers increased capacity.
► Good high current capability
► Long cycle life
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Lithium-Ion
► Lighter yet provide higher capacities
► High current capability
► Long cycle life
► Overheating will damage the batteries and cause a fire
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Lead-Acid
► Most popular rechargeable batteries worldwide
►Economical and Reliable
► Heavy and not being used for portable consumer applications.

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ᴇxᴀᴍᴘʟᴇꜱ ᴏꜰ ꜰᴜᴇʟ ᴄᴇʟʟꜱ📝

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ᴇxᴀᴍᴘʟᴇꜱ ᴏꜰ ꜰᴜᴇʟ ᴄᴇʟʟꜱ📝

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Solid Oxide Fuel Cell
↳Solid oxide fuel cells are electrochemical batteries with a solid oxide or ceramic electrolyte. They can operate at very high temperatures typically 500 to 1000 °C.  It acts as an auxiliary power unit in a wide variety of applications, such as in vehicles for stationary power generation with outputs from 100 W to 2 MW.

Oxidation or Anode Reaction:

2H₂ + 2O2− → 2H₂O + 4e−

Reduction or Cathode Reaction:
O₂ + 4e− → 2O2−

Overall Cell Reaction:
2H₂ + O₂ → 2H₂O
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Molten-Carbonate Fuel Cell

↳Molten-Carbonate fuel cells are high-temperature fuel cells that have an operational temperature of 600 °C and above. It is more cost-effective than phosphoric acid fuel cells due to metal can be a catalyst at the anode and cathode due to its high operating temperatures. It is commonly used in coal-based power plants for electrical utility, industrial, and military applications.

Oxidation or Anode Reaction:

CO32− + H2 → H2O + CO2 + 2e−

Reduction or Cathode Reaction:

CO2 + ½O2 + 2e− → CO32−

Overall Cell Reaction:

H2 + ½O2 → H2O

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ʀᴇꜰᴇʀᴇɴᴄᴇꜱ🗒️

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ʀᴇꜰᴇʀᴇɴᴄᴇꜱ🗒️

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Das, G., Choi, H., Thinh Nguyen, P. K., Kim, J., & Yoon, Y. S. (2022). Anion Exchange Membranes for Fuel Cell Application: A Review. Polymers, 14(6). https://doi.org/10.3390/polym14061197

Learning Engineering. (2020, October 30). Types of Battery | Different Types of Battery | Classification of Battery [Video]. YouTube. https://www.youtube.com/watch?v=Tye3dcBOqtY

Salah, Rabab. (2020). All about the Electrochemical Cell and its Different Types. 10.13140/RG.2.2.21520.43522.

S.S. Hosseiny, M. Wessling, 13 - Ion exchange membranes for vanadium redox flow batteries, Editor(s): Angelo Basile, Suzana Pereira Nunes, In Woodhead Publishing Series in Energy, Advanced Membrane Science and Technology for Sustainable Energy and Environmental Applications,
Woodhead Publishing, 2011, Pages 413-434, ISBN 9781845699697, https://doi.org/10.1533/9780857093790.4.413.
(https://www.sciencedirect.com/science/article/pii/B9781845699697500138)