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An example of a fuel cell is a hydrogen fuel cell. A hydrogen fuel cell creates electrical current directly from a chemical reaction. As what can be seen above, the cathode half-reaction, which is the oxygen, has undergone reduction reaction and gained 4 electrons. The hydrogen represents the anode half-reaction which has undergone oxidation process and lost 4 electrons as well. With the overall reaction obtained, the overall cell potential of this hydrogen fuel cell is 0.9 V.

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https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)/20%3A_Electrochemistry/20.7%3A_Batteries_and_Fuel_Cells

https://opentextbc.ca/chemistry/chapter/17-5-batteries-and-fuel-cells/#CNX_Chem_17_05_NiCd

https://courses.lumenlearning.com/boundless-chemistry/chapter/batteries/

https://energyfaculty.com/electrochemical-batteries/

https://opentextbc.ca/chemistryatomfirst2eopenstax/chapter/batteries-and-fuel-cells/

https://www.wattfuelcell.com/difference-between-battery-fuel-cell/

https://www.technology.matthey.com/resources/view-questions-answers/fuel-cells-batteries-similar/

https://www.differencebetween.com/difference-between-fuel-cell-and-battery/#Fuel%20Cell

https://chem.libretexts.org/Courses/can/intro/16%3A_Oxidation_and_Reduction/16.6%3A_Batteries%3A_Using_Chemistry_to_Generate_Electricity

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Example of Primary Batteries and the Redox process involved (pt. 1)

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Example of Primary Batteries and the Redox process involved (pt. 1)

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A dry cell is an example of a primary battery. As indicated in the figure above, Zn is the anode half-reaction since it lost 2 electrons and has undergone the oxidation process. While in the cathode half-reaction, the ammonium ion and manganese dioxide, gained 2 electrons and has undergone the reduction process. With this, the overall reaction obtained can be seen in the figure above and has an approximately 1.5 V overall cell potential which decreases over time.

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Batteries have 2 main classifications namely the primary and secondary batteries.

Primary batteries are batteries that are single use and not rechargeable. Here, electrode reactions are effectively irreversible, hence the reason of it to be non-rechargeable.

Secondary batteries are batteries that are rechargeable because of the reverse direction application of electrical potentials. These batteries can be recharged by the use of external circuits or sources.

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For a start, battery contains and stores energy while in fuel cells, energy is not stored. In addition, there are batteries that are rechargeable and are 'single use' that are nonrechargeable. Meanwhile in fuel cells, continuous supply of fuels and reactants is needed to generate an electric current due to the fact that the products that is formed in the reaction is being constantly removed. With this, fuel cells can provide and produce an electrical energy for a longer period of time since batteries contain a limited amount of reactants that decreases as time goes by.

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Both battery and fuel cells produces electrical energy which is caused by the chemical energy obtained from their respective chemical reactions. Also, both utilizes redox reaction to generate current that can do work- electrical energy. Lastly, the two utilizes an external circuit to allow the electron transfer of the chemical reactions happening inside of it.

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A fuel cell is a type of electrochemical cell. Similar to batteries, fuel cells convert chemical energy to electrical energy through a chemical reaction consisting of oxygen or any another oxidizing agent. To continuously produce electrical energy, constant supply of reactants or fuel, usually hydrogen, is needed. With this being said, when the reactants or fuel stops on being supplied, the reaction and process happening inside a fuel cell also eventually halts.

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Example of Secondary Batteries and the Redox process involved (pt. 1)

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Example of Secondary Batteries and the Redox process involved (pt. 1)

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An example of a secondary battery is Nickel-cadmium batteries. These batteries consist nickel-plated cathode, cadmium-plated anode, and a potassium hydroxide electrode. As indicated in the figure above, the reaction has lost and gain a total of 2 electrons. With the anode and cathode half-reactions, the overall cell potential obtained is bout 1.2 V to 1.25 V. Nickel-cadmium batteries, when properly heated, can be recharged for about 1000 times. And since cadmium is very toxic, this type of batteries shouldn't be opened and should be properly disposed.

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A battery produces an electric current; it is an electrochemical cell or is composed of series of cells. A battery utilizes chemical energy consequently producing electrical energy. With this, any galvanic cell could be utilized as a battery.

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Example of Primary Batteries and the Redox process involved (pt. 2)

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Example of Primary Batteries and the Redox process involved (pt. 2)

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Alkaline batteries are another example of a primary battery. By the name itself, alkaline batteries uses alkaline electrolytes that are often potassium hydroxide. As indicated above, the anode half-reaction has an electrical potential of -1.28 V while the cathode half-reaction has +0.15 V. Obtaining the overall chemical reaction, the overall cell potential is +1.43 V. There are alkaline batteries that are rechargeable but most of them aren't. Trying to recharge a single use alkaline battery cause leakage of potassium hydroxide and rupture of the battery itself.

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Example of Secondary Batteries and the Redox process involved (pt. 2)

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Example of Secondary Batteries and the Redox process involved (pt. 2)

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Lithium ion batteries are also an example of secondary batteries. It is one of the most popular rechargeable battery which is used in many devices that are portable. In the reaction above, you can see that there are x coefficients. Those coefficients represents moles that are not more than 0.5. With the anode and cathode half-reactions indicated in the figure, the overall cell potential or battery voltage of it is about 3.7 V.