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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.

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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. At that point, your battery is "dead."

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For batteries to work, electricity must be converted into a chemical potential form before it can be readily stored. Batteries consist of two electrical terminals called the cathode and the anode, separated by a chemical material called an electrolyte. To accept and release energy, a battery is coupled to an external circuit. Electrons move through the circuit, while simultaneously ions (atoms or molecules with an electric charge) move through the electrolyte. In a rechargeable battery, electrons and ions can move either direction through the circuit and electrolyte.

When the electrons move from the cathode to the anode, they increase the chemical potential energy, thus charging the battery; when they move the other direction, they convert this chemical potential energy to electricity in the circuit and discharge the battery. During charging or discharging, the oppositely charged ions move inside the battery through the electrolyte to balance the charge of the electrons moving through the external circuit and produce a sustainable, rechargeable system. Once charged, the battery can be disconnected from the circuit to store the chemical potential energy for later use as electricity.

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A fuel cell is a galvanic cell that requires a constant external supply of reactants because the products of the reaction are continuously removed. Unlike a battery, it does not store chemical or electrical energy; a fuel cell allows electrical energy to be extracted directly from a chemical reaction. In principle, this should be a more efficient process than, for example, burning the fuel to drive an internal

combustion engine that turns a generator, which is typically less than 40% efficient, and in fact, the efficiency of a fuel cell is generally between 40% and 60%.

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An introduction to Fuel Cells (GCSE Chemistry)

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Fuel cell is an electrochemical energy conversion device that produces electricity by combining hydrogen and oxygen into water. Like batteries, fuel cells convert potential chemical energy into electrical energy and generate heat as a by-product. However, the chemical energy is stored inside batteries—rather than generated— they can only operate for a limited duration until they need to be discarded or recharged. Fuel cells, on the other hand, can continuously generate electricity as long as they are supplied with fuel (hydrogen) and an oxidant.

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How Does a Fuel Cell Work?  │ Simple Explanation

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Fuel cells work like batteries, but they do not run down or need recharging. They produce electricity and heat as long as fuel is supplied. A fuel cell consists of two electrodes—a negative electrode (or anode) and a positive electrode (or cathode)—sandwiched around an electrolyte. A fuel, such as hydrogen, is fed to the anode, and air is fed to the cathode. In a hydrogen fuel cell, a catalyst at the anode separates hydrogen molecules into protons and electrons, which take different paths to the cathode. The electrons go through an external circuit, creating a flow of electricity. The protons migrate through the electrolyte to the cathode, where they unite with oxygen and the electrons to produce water and heat.

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College & Career Ready Labs │ Paxton Patterson

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How Does a Hydrogen Fuel Cell Work?  │ Simple Explanation

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Similarities between batteries and fuel cells

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Similarities between batteries and fuel cells

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Fuel cells are similar to batteries in that they generate an electrical current, but require continuous addition of fuel and oxidizer. The hydrogen fuel cell uses hydrogen and oxygen from the air to produce water, and is generally more efficient than internal combustion engines

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Fuel cells and batteries are both electrochemical energy storage systems that generate electricity through chemical reactions. Anodes and cathodes are included in both batteries and fuel cells, and both rely on the flow of electrons through an external circuit to produce an electrical current.

Chemical energy is captured by a battery and released as electricity. So, once a battery has drained its chemical energy, it must either be recharged or discarded. As long as it is supplied with fuel and oxygen, a fuel cell will continue to function and produce electricity.

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Differences between batteries and fuel cells

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Differences between batteries and fuel cells

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Much like a battery, a fuel cell produces electricity through electrochemical reactions, which generate electricity from hydrogen and air without any combustion. Unlike batteries, fuel cells don't need to be recharged and can continuously provide electricity as long as there's a constant source of hydrogen and oxygen

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The biggest difference between the two is that a battery stores energy, while a fuel cell takes an energy source – such as hydrogen, propane, diesel, or natural gas – and converts it into electrical energy. A fuel cell can also have a battery as a system component to store the electricity it’s generating.

Although fuel cells are predominantly used with hydrogen, they can also use fossil fuels. Rather than ‘combusting’ the fuel’s chemical energy, it ‘converts’ it. The result is a fuel cell that can create clean electricity, efficiently and effectively.

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There are two basic types of batteries: primary and secondary.

Primary batteries are “single use” and cannot be recharged. A primary battery is a convenient sources of power for portable electronics and devices. This includes radios, watches, toys, lights, camera, and more.
alkaline batteries, which use a zinc anode and a manganese dioxide cathode, and zinc-carbon batteries, which use a zinc anode and a carbon cathode are examples of primary batteries.

The second type is rechargeable and is called a secondary battery. Secondary batteries usually cost more than primary ones. But considering they’re rechargeable, they can have a longer lifespan.
Examples are Nickel – Cadmium Batteries, One of the oldest battery types available today. They have a very long life and are also very reliable and sturdy. And Nickel – Metal Hydride Batteries, They’re a new type of battery, an extended version of Nickel – Hydrogen Electrode Batteries. Ideal use in aerospace applications (satellites)

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Primary batteries are single-use batteries because they cannot be recharged. A common primary battery is the dry cell. The dry cell is a zinc-carbon battery. The zinc can serves as both a container and the negative electrode. The positive electrode is a rod made of carbon that is surrounded by a paste of manganese(IV) oxide, zinc chloride, ammonium chloride, carbon powder, and a small amount of water. The reaction at the anode can be represented as the ordinary oxidation of zinc:

Zn(s)⟶Zn2+(aq)+2e−  E∘Zn2+/Zn=−0.7618V

The reaction at the cathode is more complicated, in part because more than one reaction occurs. The series of reactions that occurs at the cathode is approximately

2MnO2(s)+2NH4Cl(aq)+2e−⟶Mn2O3(s)+2NH3(aq)+H2O(l)+2Cl−

The overall reaction for the zinc–carbon battery can be represented as

2MnO2(s)+2NH4Cl(aq)+Zn(s)⟶
Zn2+(aq)+Mn2O3(s)+2NH3(aq)+H2O(l)+2Cl−

with an overall cell potential which is initially about 1.5 V, but decreases as the battery is used. It is important to remember that the voltage delivered by a battery is the same regardless of the size of a battery.

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Nickel-cadmium, or NiCd, batteries consist of a nickel-plated cathode, cadmium-plated anode, and a potassium hydroxide electrode. The positive and negative plates, which are prevented from shorting by the separator, are rolled together and put into the case. This is a “jelly-roll” design and allows the NiCd cell to deliver much more current than a similar-sized alkaline battery. The reactions are

anode: Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−

cathode: NiO2(s)+2H2O(l)+2e−⟶Ni(OH)2(s)+2OH−(aq)
______________
overall: Cd(s)+NiO2(s)+2H2O(l)⟶Cd(OH)2(s)+Ni(OH)2(s)

The voltage is about 1.2 V to 1.25 V as the battery discharges. When properly treated, a NiCd battery can be recharged about 1000 times. Cadmium is a toxic heavy metal so NiCd batteries should never be opened or put into the regular trash.

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In a fuel cell, the fuel is oxidized at the anode which yields electrons that flow through an external circuit doing electrical work, before an oxidant (often oxygen) is reduced by these electrons at the cathode.

O2(g)+H2(g)→2H2O(l)

The resulting electricity can be used in a variety of ways, including: powering motor vehicles, electrical devices, and airplanes. Examples of fuel cells are

Alkaline Fuel Cells (AFC): AFC's use alkaline electrolytes like potassium hydroxide. Generally, a solution of potassium hydroxide in water is used as the electrolyte. The cell operates at 150-200 degrees Celsius, and can generate anywhere from 300 W to 5 MW. AFC's were first used in the Apollo Space Missions by NASA.

Molten Carbonate Fuel Cells (MCFC): MCFC's use molten carbonate salts as their electrolyte. This fuel cell has a high electrical efficiency of 60 %. These cells operate at about 600 degrees Celsius. The generated power varies, and some units have been built with outputs as high as 100 MW. Because of the high temperatures, these cells are not generally used in the home.

Zinc Air Fuel Cells (ZAFC): In this type of fuel cell, there is a gas diffusion electrode, a zinc anode separated by electrolyte and a mechanical separator. Oxygen is reduced to hydroxide, which combines with oxidized zinc, generating electrons in the process.

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The operating temperature of alkaline fuel cells range between room temperature to approximately 250 ˚C and can achieve power-generating efficiencies of up to 70 percent. A diagram of the alkaline fuel cell is shown in Figure 1. The chemical reactions that occur in an AFC are as follows:

Anode: 2H₂ (g) + 4(OH)- (aq) → 4H₂O (l) + 4e-

Cathode: O₂ (g) + 2H₂O (l)+ 4e- → 4(OH)-(aq)

Overall: 2H₂ (g) + O₂ (g) → 2H₂O (l)

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The molten carbonate fuel cell operates at approximately 650 °C (1200 °F). The high operating temperature is needed to achieve sufficient conductivity of the carbonate electrolyte, yet allow the use of low-cost metal cell components. Molten carbonate fuel cells are being developed for natural gas and coal-based power plants for industrial, electrical utility, and military applications (MCFCs operate more efficiently with CO2 containing bio-fuel derived gases.
Anode: H2 + CO3 2- -> H2O + CO2 + 2e-

Cathode: ½O2 + CO2 + 2e- ->CO3 2-

Overall: H2 + ½O2 + CO2 -> H2O + CO2

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https://learn.sparkfun.com/tutorials/what-is-a-battery/all

https://www.science.org.au/curious/technology-future/batteries#:~:text=A%20battery%20is%20a%20device,be%20used%20to%20do%20work.

https://www.science.org.au/curious/technology-future/batteries

https://www.youtube.com/watch?v=MQG87a8EwzY

https://www.energy.gov/eere/fuelcells/fuel-cells#:~:text=A%20fuel%2C%20such%20as%20hydrogen,creating%20a%20flow%20of%20electricity.

https://chem.libretexts.org/Bookshelves/General_Chemistry/Chemistry_1e_(OpenSTAX)/17%3A_Electrochemistry/17.5%3A_Batteries_and_Fuel_Cells#:~:text=a%20single%20cell.-,There%20are%20two%20basic%20types%20of%20batteries%3A%20primary%20and%20secondary,is%20called%20a%20secondary%20battery.

https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Electrochemistry/Exemplars/Case_Study%3A_Battery_Types

https://www.ceb.cam.ac.uk/research/groups/rg-eme/Edu/fuelcells/types-of-fuel-cells

https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Electrochemistry/Exemplars/Case_Study%3A_Fuel_Cells