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

Piller, taşınabilir elektrik kaynağı olarak kullanılan voltaik hücrelerdir. Birincil veya şarj edilemeyen ve ikincil veya şarj edilebilir piller olarak kategorize edilirler. Ortak birincil pil kuru pildir.Anot olarak bir çinko kılıf ve manganez oksit ve amonyum klorürden oluşan nemli, asidik bir elektrolit pastasına batırılmış bir grafit katot içerir. Çinko, çinko klorüre oksitlenir ve manganez oksit, 1, 5 voltluk bir potansiyel oluşturan katı manganez okside indirgenir. Çalıştırıldığında, elektrotlar tükenerek kuru hücreler tek kullanımlık piller haline gelir.Alkalin piller benzerdir ancak raflarını ve çalışma ömürlerini uzatan bir alkalin elektrolit kullanırlar. Kurşun asitli aküler, ağırlıklı olarak otomobillerde kullanılan ikincil akülerdir. Bunlar tipik olarak seri bağlı altı elektrokimyasal hücreye sahiptir ve toplam 12 voltluk bir potansiyel oluşturur.Her hücrede, sülfürik aside batırılmış bir kurşun anot ve bir kurşun oksit katodu bulunur. Deşarj sırasında, redoks reaksiyonları, harici bir güç kaynağı kullanılarak yeniden şarj sırasında geri dönüştürülen her iki elektrotta katı kurşun sülfat bırakır. Nikel-kadmiyum şarj edilebilir piller bir nikel oksihidroksit katot, bir kadmiyum anot ve bir potasyum hidroksit elektrolit içerir.Çalıştırıldığında, anot katı kadmiyum hidroksite oksitlenir ve katot katı nikel hidroksite indirgenerek 1, 3 voltluk bir hücre potansiyeli oluşturur. Ancak kadmiyum toksisitesi, nikel-kadmiyum pillerin çevre dostu nikel-metal hidrit pillerle değiştirilmesine neden olmuştur. Burada katot aynı kalır, ancak anot hidrojen emici bir alaşımdır.Anodik reaksiyon, hidrojenden su oluşumunu içerir. Lityum iyon piller en yeni ikincil pillerdir. Hafif lityum metal, bu pilleri yüksek enerji yoğunluğu ile taşınabilir hale getirir.Bir lityum iyon pil, lityumlanmış bir grafit anot ve bir lityum geçiş metal oksit katodu içerir. Yüklendiğinde, geçiş metali oksitlenirken, lityum iyonları anodik grafit tabakaları arasına dahil edilir. Boşalmanın ardından, lityum iyonları anottan katoda akarak 3, 7 Voltluk bir potansiyel oluşturur.Son olarak, yakıt hücreleri, enerji üretimi için sürekli bir harici redoks reaktant kaynağı gerektiren voltaik hücrelerdir. Tipik bir hidrojen yakıt hücresi, su yayarken bir akım oluşturmak için havadan hidrojen ve oksijeni kullanır. Grafit elektrotlar, redoks reaksiyonunu hızlandırmak için platin bazlı katalizörler içerir.

piller ve yakıt hücreleri

Pil, belirli uygulamalar için bir elektrik kaynağı olarak kullanılan bir galvanik hücredir. Modern piller, kol saatlerine güç verenler gibi küçük düğme pillerden belediye elektrik şebekelerine yedek enerji sağlamak için kullanılan çok büyük pillere kadar çeşitli uygulamaları barındırmak için çok sayıda formda bulunur. Bazı piller tek kullanımlık uygulamalar için tasarlanmıştır ve şarj edilemez (birincil hücreler), diğerleri ise harici bir güç kaynağı (ikincil hücreler) tarafından şarj edilmesine izin veren uygun şekilde geri dönüşümlü hücre reaksiyonlarına dayanır.
 
 Tek Kullanımlık (Birincil) Piller
 
 Kuru hücre, hem kap hem de anot (“–” terminal) olarak çinko ve katot (“+” terminali) olarak grafit çubuk kullanan yaygın bir birincil pildir. Zn kutusu, manganez(IV) oksit, çinko(II) klorür, amonyum klorür ve su içeren bir elektrolit macunu ile doldurulur. Hücreyi tamamlamak için elektrolit macununa bir grafit çubuk batırılır. Spontan hücre reaksiyonu şunları içerir:
 
 <img alt="Eq1" src="/files/ftp_upload/11439/11439_Equation_1.png" style="text-align: center; height: 168px;" />
 
 Kuru bir hücrenin voltajı (hücre potansiyeli) yaklaşık 1,5 V'dir (Ehücre ~ 1,5 V). Kuru hücreler çeşitli boyutlarda mevcuttur (örneğin, D, C, AA, AAA). Tüm kuru hücre boyutları aynı bileşenleri içerir ve aynı voltajı gösterir, ancak daha büyük hücreler daha fazla miktarda redoks reaktanları içerir ve bu nedenle buna bağlı olarak daha fazla miktarda yük aktarabilir. Diğer galvanik hücreler gibi, kuru hücreler de gerekirse daha büyük voltaj çıkışlarına sahip piller elde etmek için seri olarak bağlanabilir.
 
 Alkalin piller, kuru hücre ile aynı redoks çiftleri etrafında tasarlanmıştır. Adından da anlaşılacağı gibi, bu tür piller genellikle potasyum hidroksit olan alkalin elektrolitler kullanır. Reaksiyonları şunlardır
 
 <img alt="Eq2" src="/files/ftp_upload/11439/11439_Equation_2.png" style="text-align: center; height: 130px;" />
 
 Bir alkalin pil, benzer boyuttaki kuru bir hücrenin yaklaşık üç ila beş katı enerji sağlayabilir (Ehücre  = +1,43 V). Alkalin piller potasyum hidroksit sızıntısına eğilimlidir, bu nedenle uzun süreli depolama için cihazlardan çıkarılmalıdır. Bazı alkalin piller şarj edilebilir olsa da, çoğu değildir.
 
 Şarj Edilebilir (İkincil) Piller
 
 Nikel-kadmiyum veya NiCd piller, nikel kaplı bir katot, kadmiyum kaplı anot ve bir potasyum hidroksit elektrotundan oluşur. Ayırıcı tarafından kısa devre yapılmasını önleyen pozitif ve negatif plakalar bir araya getirilir ve kasaya konur. Bu tasarım, NiCd hücresinin benzer büyüklükteki bir alkalin pilden çok daha fazla akım vermesini sağlar. Reaksiyonları şunlardır
 
 <img alt="Eq3" src="/files/ftp_upload/11439/11439_Equation_3.png" style="text-align: center; height: 130px;" />
 
 Uygun şekilde muamele edildiğinde, bir NiCd pil yaklaşık 1000 kez şarj edilebilir (Ehücre ~ 1,3 V). Kadmiyum toksik bir ağır metaldir, bu nedenle NiCd piller asla yırtılmamalı veya yakılmamalı ve ilgili toksik atık yönergelerine uygun olarak atılmalıdır.
 
 Lityum-iyon piller en popüler şarj edilebilir piller arasındadır ve birçok taşınabilir elektronik cihazda kullanılır. Reaksiyonları şunlardır
 
 <img alt="Eq4" src="/files/ftp_upload/11439/11439_Equation_4.png" style="text-align: center; height: 130px;" />
 
 Hücre reaksiyonunun değişken stokiyometrisi, hücre voltajlarında değişime yol açar, ancak tipik koşullar için, x genellikle 0,5'ten fazla değildir ve hücre voltajı yaklaşık 3,7 V'tur (Ehücre ~ 3,7). Lityum piller popülerdir, çünkü büyük miktarda akım sağlayabilirler, diğer tipteki benzer pillerden daha hafiftirler, boşaldıkça neredeyse sabit bir voltaj üretirler ve depolandığında şarjlarını yavaş yavaş kaybederler.
 
 Kurşun-asit akü aynı zamanda otomobillerde yaygın olarak kullanılan bir ikincil akü türüdür. Ucuzdur ve otomobil marş motorlarının ihtiyaç duyduğu yüksek akımı üretebilir. Bir kurşun-asit batarya için reaksiyonlar şunlardır
 
 <img alt="Eq5" src="/files/ftp_upload/11439/11439_Equation_5.png" style="text-align: center; height: 160px;" />
 
 Her hücre 2 V (Ehücre ~ 2 V) üretir, bu nedenle 12 V'luk bir araç aküsü üretmek için altı hücre seri olarak bağlanır. Kurşun-asit piller ağırdır ve kostik bir sıvı elektrolit, H2SO4 (aq) içerir, ancak yüksek akım yoğunluğu nedeniyle genellikle hala tercih edilen pillerdir. Bu piller önemli miktarda kurşun içerdiğinden, her zaman düzgün bir şekilde atılmalıdır.
 
 Yakıt Hücreleri
 
 Bir yakıt hücresi, bir oksidan ile birlikte hücreye sürekli olarak beslenen geleneksel yanıcı yakıtları, çoğunlukla hidrojen veya metanı kullanan bir galvanik hücredir. Hücre içinde, yakıt ve oksidan, yandıklarında olduğu gibi aynı redoks kimyasına maruz kalırlar, ancak önemli ölçüde daha verimli olan katalize edilmiş bir elektrokimyasal vasıtasıyla gerçekleşir. Örneğin, tipik bir hidrojen yakıt hücresi, iki yarım hücre reaksiyonunu hızlandırmak için platin bazlı katalizörlerle gömülü grafit elektrotları kullanır:
 
 <img alt="Eq6" src="/files/ftp_upload/11439/11439_Equation_6.png" style="text-align: center; height: 130px;" />
 
 Bu tip yakıt hücreleri genellikle yaklaşık 1,23 V (Ehücre ~ 1,23 V) voltaj üretir. Bir içten yanmalı motorla karşılaştırıldığında, aynı redoks reaksiyonunu kullanan bir yakıt hücresinin enerji verimliliği tipik olarak iki kattan fazladır (bir motor için ~20%–25%, bir yakıt hücresi için ~50%–75%). Hidrojen yakıt hücreleri, genişletilmiş uzay görevlerinde yaygın olarak kullanılmaktadır ve kişisel araçlar için prototipler geliştirilmiştir.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/17-5-batteries-and-fuel-cells">Openstax, Chemistry 2e, Section 17.5: Batteries, and Fuel Cells.</a>

Piller ve Yakıt Hücreleri

Pil, belirli uygulamalar için elektrik gücü kaynağı olarak kullanılan galvanik bir hücredir. Modern piller çok çeşitli biçimlerde bulunur ...

Education

JoVE Core

Chemistry

Kimya

Electrochemistry

Elektrokimya

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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...

electromotive force

Cell Voltage and Electron Flow

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...

voltaic/galvanic cells

Galvanic Cells and Battery Reactions

Galvanic cells use spontaneous redox reactions to produce electric current. A common example is a disposable AA battery, which powers devices by turning chemical energy into electrical energy. Another example is a copper wire placed in silver nitrate solution, where the solution slowly turns bright blue and a grey solid forms on the wire. In the copper and silver reaction, copper is oxidized and silver ions are reduced. Copper forms cuprous ions, which give the solution its blue color. At the...

standard electrode potentials

Using Electrode Potentials to Predict Reactions

Electrode potentials help predict whether a redox reaction will happen on its own. A redox reaction involves electron transfer. In electrochemistry, the measured value is called cell potential or cell voltage. It shows the energy linked to charge transfer and is measured in volts, where 1 volt equals 1 joule per coulomb. A single half-cell cannot be measured by itself because electron transfer needs both a donor and a receiver. For that reason, scientists measure the difference between two...

cell potential and free energy

Redox Cell Potential, ΔG°, and K

Redox cell potential connects chemical energy, free energy change, and the equilibrium constant in an electrochemical cell. In these reactions, chemical energy is converted into electrical energy. That link helps predict whether a reaction is spontaneous and how far it may proceed. Thermodynamics is the study of how heat and other forms of energy are related. In an electrochemical cell, cell potential can also reflect oxidizing strength or reducing strength. A similar idea appears in acid-base...

the nernst equation

Cell Potential Under Changing Conditions

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...

concentration cells

Cell Potential from Concentration Differences

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

Rusting and Metal Protection

Corrosion is the natural breakdown of metals through electrochemical reactions. It can appear as rust on iron, tarnish on silver, or a blue-green patina on copper. In each case, the metal is oxidized. Some corrosion products can protect the surface, while others keep damaging the metal. Rusting is the harmful type of corrosion seen in iron. It happens when iron is exposed to oxygen and water. A galvanic cell forms on the iron surface, and this drives oxidation at the anodic region and...

electrolysis

Electrolysis in Batteries and Metal Production

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

chemistry

JoVE Core Kimya, özlü ve kolay anlaşılır animasyon video derslerini kullanarak genel kimya kavramlarına hayat veriyor. Ek olarak, bilim insanı uygulama videolarımız ile klasik ve orijinal araştırma deneylerini dünya çapında günümüz laboratuvarlarında görselleştiriyoruz.

Louisiana Student Standards for Science

High School

motion-and-stability-forces-and-interactions

Motion And Stability: Forces And Interactions

HS-PS2-5

Physics

Arizona Science Standards

HS.P1

HS.P1U3.4

HS+Phy.P4

HS+Phy.P4U2.7

HS.P4

HS.P4U3.9

Alabama Course of Study Science

Matter and Its Interactions

9-12.PS.3.4

Next Generation Science Standards

Motion and Stability: Forces and Interactions

Texas Essential Knowledge and Skills

PHYS.6

PHYS.6.D

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

Energy

P-PS3-3

Newton's Second Law

Newton&#39;s second law is closely related to his first law of motion. It mathematically gives the cause-and-effect relationship between force and changes ...

Second Law: Motion under Same Force

Newton&#39;s laws can be applied to bodies at rest and bodies in motion. Newton&#39;s first law is applied to bodies in equilibrium, whereas the second ...

second-law-motion-under-same-acceleration

Second Law: Motion under Same Acceleration

Newton&#39;s second law of motion applies to bodies moving under the same acceleration. For example, when a baggage tractor pulls luggage carts, each cart ...

Students who demonstrate understanding can analyze data to support the claim that Newton's second law of motion describes the mathematical relationship among the net force on a macroscopic object, its mass, and its acceleration.  Clarifying Statement: Examples of data could include tables or graphs of position or velocity as a function of time for objects subject to a net unbalanced force, such as a falling object, an object sliding down a ramp, or a moving object being pulled by a constant force.  Assessment Boundry: Assessment is limited to one-dimensional motion and to macroscopic objects moving at non-relativistic speeds.

3.2.9-12.I

Inertial Frames of Reference

Newton&#8217;s first law is usually considered to be a statement about reference frames. It provides a method for identifying a special type of reference ...

Non-inertial Frames of Reference

A reference frame accelerating or decelerating relative to an inertial frame is a non-inertial frame. To help understand this, consider what taking off in ...

Linear Momentum

The term momentum is used in various ways in everyday language, most of which are consistent with the precise scientific definition. Generally, momentum ...

Conservation of Momentum: Introduction

The total momentum of a system consisting of N interacting objects is constant in time or is conserved. A system must meet two requirements for its ...

Conservation of Momentum: Problem Solving

Solving problems using the conservation of momentum requires four basic steps:

	Identify a closed system, where the total mass is constant, and no net ...

Students who demonstrate understanding can use mathematical representations to support the claim that the total momentum of a system of objects is conserved when there is no net force on the system.  Clarifying Statement: Emphasis is on the quantitative conservation of momentum in interactions and the qualitative meaning of this principle.  Assessment Boundry: Assessment is limited to systems of two macroscopic bodies moving in one dimension.

3.2.9-12.J

Students who demonstrate understanding can apply scientific and engineering ideas to design, evaluate and refine a device that minimizes the force on a macroscopic object during a collision. Clarifying Statement: Examples of evaluation and refinement could include determining the success of the device at protecting an object from damage and modifying the design to improve it. Examples of a device could include a football helmet or a parachute. Assessment Boundry: Assessment is limited to qualitative evaluations and/or algebraic manipulations.

3.2.9-12.K

Gravitation

In the years before Newton, a general belief prevailed that different laws governed objects in the sky than objects on Earth. When Kepler wrote down the ...

/files/media/science-education/science-education-thumbs/14716.jpg

Newton's Law of Gravitation

Our everyday observation tells us that all objects close to the Earth naturally tend to fall to the ground. Early philosophers assumed that this downward ...

Electric Charges

From lightning during thunderstorms to electronic devices, the phenomenon of electromagnetism is all around us. The electromagnetic force is one of the ...

sources-and-properties-of-electric-charge

Sources and Properties of Electric Charge

All objects we see around us consist of atoms, which combine to form molecules. The lightest element in the universe is hydrogen, and a hydrogen atom ...

Coulomb's Law

Experiments with electric charges have shown that if two objects each have an electric charge, they exert an electric force on each other. The magnitude ...

the-principle-of-superposition-and-the-gravitational-field

The Principle of Superposition and the Gravitational Field

The principle of superposition applies to gravitational forces of objects that are sufficiently far apart. It states that the net gravitational force on a ...

/files/media/science-education/science-education-thumbs/14754.jpg

Electric Field

Consider two point charges, each exerting Coulomb force on the other. It is possible to describe the Coulomb interaction via an intermediate step by ...

Magnetic Fields

A moving charge or a current creates a magnetic field in the surrounding space, in addition to its electric field. The magnetic field exerts a force on ...

Magnetic Field due to Moving Charges

A stationary charge creates and interacts with the electric field, while a moving charge creates a magnetic field.
Consider a point charge moving with a ...

Electromagnetic Fields

Electric fields generated by static charges, often referred to as electrostatic fields, are characteristically different from electric fields created by ...

Students who demonstrate understanding can use mathematical representations of Newton's Law of Gravitation and Coulomb's Law to describe and predict the gravitational and electrostatic forces between objects. Clarifying Statement: Emphasis is on both quantitative and conceptual descriptions of gravitational and electric fields. Assessment Boundry: Assessment is limited to systems with two objects.

3.2.9-12.L

Energy Transfer in Chemical Reactions

Chemical reactions require sufficient energy to cause the matter to collide with enough precision and force that old chemical bonds can be broken and new ...

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 ...

Students who demonstrate understanding can plan and conduct an investigation to provide evidence that an electric current can produce a magnetic field and that a changing magnetic field can produce an electric current. Clarifying Statement: N/A Assessment Boundry: Assessment is limited to designing and conducting investigations with provided materials and tools.

Primary, Rechargeable Batteries and Fuel Cells

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