Name: primary, rechargeable batteries and fuel cells
Uploaded: 2020-09-24T15:06:52.000Z
Duration: 3 min 12 s
Channel: JoVE

K12 Standards

Pennsylvania State Academic Standards

9-12

Physical Science

Forces and Interactions

3.2.9-12.M

Batteries and Fuel Cells

Batterijen zijn volta cellen die worden gebruikt als draagbare elektrische bronnen. Ze worden onderverdeeld in primaire of niet-oplaadbare en secundaire of oplaadbare batterijen. De gemeenschappelijke primaire batterij is de droge cel.Het bevat een zinkomhulsel als anode en een grafietkathode ondergedompeld in een vochtige, zure elektrolytpasta van mangaan(IV)oxide en ammoniumchloride. Het zink oxideert tot zinkchloride en mangaan(IV)oxide reduceert tot vast mangaan(III)oxide en genereert een potentiaal van 1, 5 volt. Bij gebruik raken de elektroden uitgeput, waardoor droge cellen batterijen voor eenmalig gebruik zijn.Alkalinebatterijen lijken hierop, maar gebruiken een alkalische elektrolyt om hun houdbaarheid en levensduur te verlengen. Loodzuurbatterijen zijn secundaire batterijen die voornamelijk in auto's worden gebruikt. Deze hebben doorgaans zes elektrochemische cellen die in serie zijn geschakeld en een totaal potentiaal van 12 volt genereren.Elke cel heeft een loden anode en een loodoxidekathode ondergedompeld in zwavelzuur. Tijdens het ontladen zetten de redoxreacties vast loodsulfaat af op beide elektroden, die tijdens het opladen weer worden omgezet met behulp van een externe stroombron. Oplaadbare nikkel-cadmiumbatterijen bevatten een nikkeloxyhydroxidekathode, een cadmiumanode en een kaliumhydroxide-elektrolyt.Bij gebruik oxideert de anode tot vast cadmiumhydroxide en de kathode reduceert tot vast nikkelhydroxide, waardoor een celpotentiaal van 1, 3 volt wordt gegenereerd. De giftigheid van cadmium stimuleert echter de vervanging van nikkel-cadmiumbatterijen door milieuvriendelijke nikkel-metaalhydride-batterijen. Hier blijft de kathode hetzelfde, maar de anode is een waterstofabsorberende legering.De anodische reactie omvat de vorming van water uit waterstof. Lithium-ionbatterijen zijn de nieuwste secundaire batterijen. Lichtgewicht lithiummetaal maakt deze batterijen draagbaar met een hoge energiedichtheid.Een lithium-ionbatterij bevat een anode van gelithieerd grafiet en een kathode van lithiumovergangsmetaaloxide. Wanneer geladen, wordt het overgangsmetaal geoxideerd, terwijl lithiumionen worden opgenomen tussen de anodische grafietlagen. Bij ontlading stromen lithiumionen van de anode naar de kathode en genereren een potentiaal van 3, 7 volt.Ten slotte zijn brandstofcellen volta cellen die een continue externe toevoer van redoxreactanten nodig hebben voor energieproductie. Een typische waterstof-brandstofcel gebruikt waterstof en zuurstof uit de lucht om een stroom op te wekken terwijl ze water uitstoten. Grafietelektroden bevatten op platina gebaseerde katalysatoren om de redoxreactie te versnellen.

batterijen en brandstofcellen

Een batterij is een galvanische cel die wordt gebruikt als elektrische energiebron voor specifieke toepassingen. Moderne batterijen bestaan in een groot aantal vormen voor verschillende toepassingen, van kleine knoopbatterijen zoals die voor polshorloges tot de zeer grote batterijen die worden gebruikt om reserve-energie te leveren aan gemeentelijke elektriciteitsnetten. Sommige batterijen zijn ontworpen voor toepassingen voor eenmalig gebruik en kunnen niet worden opgeladen (primaire cellen), terwijl andere gebaseerd zijn op handig omkeerbare celreacties die opladen door een externe stroombron mogelijk maken (secundaire cellen). (Primaire) batterijen voor eenmalig gebruik Een droge cel is een gewone primaire batterij die zink gebruikt als zowel de container als de anode (“–” aansluiting) en een grafietstaaf als de kathode (“+” aansluiting). Het zinkblik is gevuld met een elektrolytpasta die mangaan (IV) oxide, zink (II) chloride, ammoniumchloride en water bevat. Een grafietstaaf wordt ondergedompeld in de elektrolytpasta om de cel te voltooien. De spontane celreactie omvat: <img alt="Eq1" src="/files/ftp_upload/11439/11439_Equation_1.png" style="text-align: center; height: 168px;"> De spanning (celpotentiaal) van een droge cel is ongeveer 1,5 V (Ecell ~ 1,5 V). Droge cellen zijn verkrijgbaar in verschillende maten (bijvoorbeeld D, C, AA, AAA). Alle maten droge cellen bevatten dezelfde componenten en vertonen dezelfde spanning, maar grotere cellen bevatten grotere hoeveelheden redoxreagentia en zijn daarom in staat overeenkomstig grotere hoeveelheden lading over te dragen. Net als andere galvanische cellen kunnen droge cellen in serie worden geschakeld om, indien nodig, batterijen met een grotere spanningsuitgang te leveren. Alkalinebatterijen zijn ontworpen rond dezelfde redoxkoppels als de droge cel. Zoals hun naam doet vermoeden, gebruiken dit soort batterijen alkalische elektrolyten, vaak kaliumhydroxide. De reacties zijn <img alt="Eq2" src="/files/ftp_upload/11439/11439_Equation_2.png" style="text-align: center; height: 130px;"> Een alkalische batterij kan ongeveer drie tot vijf keer de energie leveren van een droge cel van vergelijkbare grootte (Ecell = +1,43 V). Alkalinebatterijen zijn gevoelig voor het lekken van kaliumhydroxide en moeten daarom uit apparaten worden verwijderd voor langdurige opslag. Hoewel sommige alkalibatterijen oplaadbaar zijn, zijn de meeste dat niet. Oplaadbare (secundaire) batterijen Nikkel-cadmium- of NiCd-batterijen bestaan uit een vernikkelde kathode, een met cadmium beklede anode en een kaliumhydroxide-elektrode. De positieve en negatieve platen, die door de scheider voorkomen dat er kortsluiting ontstaat, worden opgerold en in de behuizing geplaatst. Dankzij dit ontwerp kan de NiCd-cel veel meer stroom leveren dan een alkalische batterij van vergelijkbare grootte. De reacties zijn <img alt="Eq3" src="/files/ftp_upload/11439/11439_Equation_3.png" style="text-align: center; height: 130px;"> Bij juiste behandeling kan een NiCd-batterij ongeveer 1000 keer worden opgeladen (Ecell ~ 1,3 V). Cadmium is een giftig zwaar metaal, dus NiCd-batterijen mogen nooit worden gescheurd of verbrand, en moeten worden weggegooid in overeenstemming met de relevante richtlijnen voor giftig afval. Lithium-ionbatterijen behoren tot de meest populaire oplaadbare batterijen en worden in veel draagbare elektronische apparaten gebruikt. De reacties zijn <img alt="Eq4" src="/files/ftp_upload/11439/11439_Equation_4.png" style="text-align: center; height: 130px;"> De variabele stoichiometrie van de celreactie leidt tot variatie in celspanningen, maar voor typische omstandigheden is x gewoonlijk niet meer dan 0,5, en is de celspanning ongeveer 3,7 V (Ecell ~ 3,7). Lithiumbatterijen zijn populair omdat ze een grote hoeveelheid stroom kunnen leveren, lichter zijn dan vergelijkbare batterijen van andere typen, een vrijwel constante spanning produceren tijdens het ontladen en slechts langzaam hun lading verliezen als ze worden opgeslagen. De loodzuuraccu is ook een type secundaire accu dat veel in auto's wordt gebruikt. Het is goedkoop en kan de hoge stroom produceren die nodig is voor startmotoren van auto's. De reacties voor een loodzuuraccu zijn: <img alt="Eq5" src="/files/ftp_upload/11439/11439_Equation_5.png" style="text-align: center; height: 160px;"> Elke cel produceert 2 V (Ecell ~ 2 V), dus zes cellen worden in serie geschakeld om een auto-accu van 12 V te produceren. Loodzuuraccu's zijn zwaar en bevatten een bijtende vloeibare elektrolyt, H2SO4 (aq), maar zijn vanwege hun hoge stroomdichtheid vaak nog steeds de voorkeursaccu. Omdat deze batterijen een aanzienlijke hoeveelheid lood bevatten, moeten ze altijd op de juiste manier worden weggegooid. Brandstofcellen Een brandstofcel is een galvanische cel die traditionele verbrandingsbrandstoffen gebruikt, meestal waterstof of methaan, die samen met een oxidatiemiddel continu in de cel worden gevoerd. Binnen de cel ondergaan brandstof en oxidatiemiddel dezelfde redoxchemie als wanneer ze worden verbrand, maar via een gekatalyseerde elektrochemische stof die aanzienlijk efficiënter is. Een typische waterstofbrandstofcel maakt bijvoorbeeld gebruik van grafietelektroden ingebed met op platina gebaseerde katalysatoren om de twee halfcelreacties te versnellen: <img alt="Eq6" src="/files/ftp_upload/11439/11439_Equation_6.png" style="text-align: center; height: 130px;"> Dit soort brandstofcellen produceren doorgaans spanningen van ongeveer 1,23 V (Ecell ~ 1,23 V). Vergeleken met een verbrandingsmotor is de energie-efficiëntie van een brandstofcel die dezelfde redoxreactie gebruikt doorgaans meer dan het dubbele (~20%–25% voor een motor versus ~50%–75% voor een brandstofcel). Waterstofbrandstofcellen worden vaak gebruikt bij uitgebreide ruimtemissies en er zijn prototypes voor persoonlijke voertuigen ontwikkeld.

Batterijen en brandstofcellen

A battery is a galvanic cell that is used as a source of electrical power for specific applications. Modern batteries exist in a multitude of forms to ...

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primary, rechargeable batteries and fuel cells

Batteries and fuel cells are galvanic cells that supply electrical power for many applications. They range from tiny button batteries in wristwatches to large systems that can provide backup energy to municipal power grids. Some are primary cells, which are single-use and cannot be recharged. Others are secondary cells, which use reversible reactions and can be charged again by an external power source.

A common primary battery is the dry cell. It uses zinc as both the container and the anode, or negative terminal, and a graphite rod as the cathode, or positive terminal. The zinc can holds an electrolyte paste with manganese(IV) oxide, zinc(II) chloride, ammonium chloride, and water. A dry cell has a voltage of about 1.5 V. It comes in sizes such as D, C, AA, and AAA. These sizes use the same parts and the same voltage, but larger cells contain more reactants and can transfer more charge. Dry cells can also be connected in series to increase voltage.

Alkaline batteries use the same redox couples as dry cells, but they use an alkaline electrolyte, often potassium hydroxide. They can deliver about three to five times the energy of a dry cell of similar size and have a cell potential of about 1.43 V. These batteries can leak potassium hydroxide, so they should be removed from devices during long-term storage. Some alkaline batteries are rechargeable, but most are not.

Rechargeable batteries include nickel-cadmium, or NiCd, batteries, lithium-ion batteries, and lead-acid batteries. A NiCd battery has a nickel-plated cathode, a cadmium-plated anode, and a potassium hydroxide electrode. The positive and negative plates are rolled together with a separator to keep them from shorting. This design lets a NiCd cell deliver much more current than a similar-sized alkaline battery. When treated properly, it can be recharged about 1000 times, and its cell potential is about 1.3 V. Cadmium is toxic, so NiCd batteries should not be ruptured or burned and must be disposed of as toxic waste.

Lithium-ion batteries are widely used in portable electronic devices. Their reaction has variable stoichiometry, so the voltage can vary, but under typical conditions the cell potential is about 3.7 V. These batteries are popular because they can provide a large amount of current, are lighter than comparable batteries of other types, and keep a nearly constant voltage as they discharge. They also lose charge slowly during storage. Lead-acid batteries are common in automobiles. They are inexpensive and can deliver the high current needed by starter motors. Each cell produces 2 V, so six cells are connected in series to make a 12-V car battery. These batteries are heavy and contain a caustic sulfuric acid electrolyte, and they also contain a significant amount of lead, so they must be disposed of properly.

A fuel cell is also a galvanic cell, but it uses a fuel that is continuously fed into the cell along with an oxidant. The fuel is often hydrogen or methane. Inside the cell, the same redox chemistry that occurs in combustion is carried out by a catalyzed electrochemical process that is much more efficient. A typical hydrogen fuel cell uses graphite electrodes with platinum-based catalysts to speed the half-cell reactions. These fuel cells usually produce about 1.23 V. Compared with an internal combustion engine, a fuel cell using the same redox reaction is typically more than twice as efficient. Hydrogen fuel cells are used on extended space missions, and prototypes for personal vehicles have been developed.

Primary, Rechargeable Batteries and Fuel Cells

primary-rechargeable-batteries-and-fuel-cells

balancing redox equations

Redox Reactions and Half-Reaction Balancing

Redox reactions involve electron transfer and changes in oxidation number. In electrochemistry, these reactions connect chemical changes with electrical energy. They also power technologies such as industrial metal processing and rechargeable batteries used in electric vehicles. Oxidation number is a way to track how an atom's electronic environment changes compared with the pure element, where the oxidation number is zero. For a simple ionic compound, the oxidation number matches the ion...

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Electric current is the flow of electric charge through a conducting medium or a solution. In wires, that charge is carried by electrons. In some solutions, ions can also move and carry charge. When electrons move through a wire, they produce an electric current. This idea connects to redox reactions, where electrons are lost and gained. In the spontaneous reaction between zinc and copper ions, zinc is oxidized to zinc ions. Copper ions are reduced to solid copper. Even so, this direct...

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Cell potential changes when a redox reaction does not run at standard conditions. Standard cell potentials connect with standard free energy change, ΔG°, and the equilibrium constant K, but those relationships only hold at 1 M concentration, 298 K, and 1 atmosphere. A zinc(II) and tin(II) redox cell with E°cell = +0.291 V and ΔG° = −56.2 kJ is spontaneous under those standard conditions. As a cell discharges, the reactant concentration changes and the cell potential steadily drops. Many redox...

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Concentration cells are voltaic cells that use two almost identical half-cells. The half-cells use the same electrode and the same half-reaction. They differ only in the concentration of one redox species, so the cell potential depends on that concentration difference. In a concentration cell, the Nernst equation can be used to find the cell potential. For the zinc example shown, the calculated cell potential is positive. A positive cell potential means the overall reaction is spontaneous. <br...

batteries and fuel cells

Batteries and fuel cells are galvanic cells that supply electrical power for many applications. They range from tiny button batteries in wristwatches to large systems that can provide backup energy to municipal power grids. Some are primary cells, which are single-use and cannot be recharged. Others are secondary cells, which use reversible reactions and can be charged again by an external power source. A common primary battery is the dry cell. It uses zinc as both the container and the anode,...

corrosion

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Electrolysis uses electrical energy to drive a nonspontaneous redox reaction. In a galvanic cell, a spontaneous redox reaction does electrical work on the surroundings by sending electrons through an external circuit. In electrolysis, an external circuit does work on the redox system by applying a voltage large enough to force the reaction in the opposite direction. This process is used in several real-world settings. Recharging a battery is one example, because an outside power source drives...

key terms and concepts

Explore dry cells, alkaline batteries, NiCd, lithium-ion, and lead-acid batteries, plus how hydrogen fuel cells turn fuel into electricity more efficiently.

Primary, Rechargeable Batteries and Fuel Cells | JoVE K12

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3.2.9-12.J

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3.2.9-12.L

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Primary, Rechargeable Batteries and Fuel Cells

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