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

Les batteries sont des cellules voltaïques utilisées comme sources électriques portables. Ils sont classés en primaire ou non rechargeable et piles secondaires ou rechargeables. La batterie principale commune est la pile sèche.Il contient un boîtier en zinc comme anode et une cathode en graphite immergé dans une pâte d'électrolyte acide et humide d'oxyde de manganèse et de chlorure d'ammonium. Le zinc s'oxyde en chlorure de zinc, et l'oxyde de manganèse se réduit en oxyde manganèse solide générant un potentiel de 1, 5 volts. Lorsqu'elles sont utilisées, les électrodes s'épuisent, ce qui rend les piles sèches à usage unique.Les piles alcalines sont similaires mais utilisent un électrolyte alcalin qui prolonge leur durée de vie et leur durée de conservation. Les batteries au plomb sont des batteries secondaires principalement utilisé dans les automobiles. Ceux-ci ont généralement six cellules électrochimiques connectés en série, générant un potentiel total de 12 volts.Chaque cellule a une anode en plomb et une cathode en oxyde de plomb immergé dans l'acide sulfurique. Lors de la décharge, les réactions redox déposent un sulfate de plomb solide sur les deux électrodes, qui sont reconvertis pendant la recharge en utilisant une source d'alimentation externe. Les piles rechargeables au nickel-cadmium contiennent une cathode oxyhydroxyde de nickel, une anode de cadmium, et un électrolyte d'hydroxyde de potassium.Lorsqu'elle est utilisée, l'anode s'oxyde en cadmium hydroxyde solide, et la cathode réduit à l'hydroxyde de nickel solide, générant un potentiel cellulaire de 1, 3 volts. Cependant, la toxicité du cadmium entraîne le remplacement de batteries nickel-cadmium par les batteries nickel-métal-hydrure plus écologiques. Ici, la cathode reste la même, mais l'anode est un alliage absorbant l'hydrogène.La réaction anodique implique la formation d'eau de l'hydrogène. Les batteries lithium-ion sont les batteries secondaires les plus récentes. Le lithium métal léger rend ces batteries portables avec une densité d'énergie élevée.Une batterie lithium-ion contient une anode en graphite lithié et une cathode d'oxyde de métal de transition au lithium. Lorsqu'il est chargé, le métal de transition est oxydé, tandis que les ions lithium sont incorporés entre les couches de graphite anodique. Lors de la décharge, les ions lithium circulent de l'anode à la cathode générant un potentiel de 3, 7 volts.Enfin, les piles à combustible sont des piles voltaïques qui nécessitent une alimentation externe continue de réactifs redox pour la production d'énergie. Une pile à hydrogène typique utilise de l'hydrogène et de l'oxygène de l'air pour générer un courant tout en émettant de l'eau. Les électrodes en graphite contiennent des catalyseurs à base de platine pour accélérer la réaction redox.

batteries et piles à combustible

Une pile est une cellule galvanique utilisée comme source d'alimentation électrique pour des applications précises. Les piles modernes existent sous de nombreuses formes pour s'adapter à diverses applications, allant des toutes petites piles boutons telles que celles qui alimentent les montres de poignet aux très grandes batteries utilisées pour fournir de l'énergie de secours aux réseaux électriques municipaux. Certaines piles sont conçues pour des applications à usage unique et ne peuvent pas être rechargées (cellules primaires), tandis que d'autres sont basées sur des réactions de cellule facilement réversibles qui permettent la recharge grâce à une source d'alimentation externe (cellules secondaires). 
 Piles à usage unique (primaires) 
 Une pile sèche est une cellule primaire courante qui utilise le zinc à la fois comme réceptacle et comme anode (borne “–”) et une tige en graphite comme cathode (borne “+”). Le boîtier en Zn est rempli d'une pâte électrolytique contenant de l'oxyde de manganèse(IV), du chlorure de zinc(II), du chlorure d'ammonium et de l'eau. Une tige en graphite est immergée dans la pâte électrolytique pour compléter la pile. La réaction spontanée de la cellule implique : 
 <img alt="Eq1" src="/files/ftp_upload/11439/11439_Equation_1.png" style="text-align: center; height: 168px;" />
 La tension (potentiel de cellule) d'une pile sèche est d'environ 1,5 V (Ecellule ~ 1,5 V). Les piles sèches sont disponibles dans des tailles différentes (par exemple, D, C, AA, AAA). Toutes les tailles de piles sèches comprennent les mêmes composants et présentent la même tension, mais les cellules plus grandes contiennent de plus grandes quantités de réactifs redox et sont donc capables de transférer des quantités de charge proportionnellement plus élevées. Comme les autres cellules galvaniques, les piles sèches peuvent être connectées en série pour produire des batteries avec des sorties de tension plus élevées, si nécessaire.  
 Les piles alcalines ont été conçues autour des mêmes couples redox que la pile sèche. Comme leur nom l'indique, ces types de piles utilisent des électrolytes alcalins, souvent de l'hydroxyde de potassium. Les réactions sont :
 <img alt="Eq2" src="/files/ftp_upload/11439/11439_Equation_2.png" style="text-align: center; height: 130px;" />
 Une pile alcaline peut fournir environ trois à cinq fois l'énergie d'une pile sèche de taille similaire (Ecellule  = +1,43 V). Les piles alcalines sont sujettes à des fuites d'hydroxyde de potassium. Elles doivent donc être retirées des dispositifs pour un stockage à long terme. Bien que certaines piles alcalines soient rechargeables, la plupart ne le sont pas. 
 Piles rechargeables (secondaires) 
 Les piles au nickel-cadmium, ou NiCd, sont constitués d'une cathode nickelé, d'une anode plaquée au cadmium et d'une électrode d'hydroxyde de potassium. Les plaques positive et négative, qui ne peuvent pas être court-circulées par le séparateur, sont enroulées ensemble et placées dans le boîtier. Cette conception permet à la cellule NiCd de fournir beaucoup plus de courant qu'une pile alcaline de taille similaire. Les réactions sont :
 <img alt="Eq3" src="/files/ftp_upload/11439/11439_Equation_3.png" style="text-align: center; height: 130px;" />
 Lorsqu'elle est correctement utilisée, une pile NiCd peut être rechargé environ 1000 fois (Ecellule ~ 1,3 V). Le cadmium est un métal lourd toxique. Par conséquent, les piles NiCd ne doivent jamais être rompues ou incinérées et on doit s'en débarrasser conformément aux directives relatives aux déchets toxiques. 
 Les piles à l'ion lithium sont parmi les piles rechargeables les plus populaires et sont utilisées dans de nombreux appareils électroniques portables. Les réactions sont :
 <img alt="Eq4" src="/files/ftp_upload/11439/11439_Equation_4.png" style="text-align: center; height: 130px;" />
 La stœchiométrie variable de la réaction des cellules entraîne une variation des tensions de cellule, mais dans des conditions usuelles, x n'est généralement pas supérieur à 0,5 et la tension de cellule est d'environ 3,7 V (Ecellule ~ 3,7). Les piles au lithium sont répandues car elles peuvent fournir une grande quantité de courant, elles sont plus légères que les autres types de piles comparables, elles produisent une tension presque constante lorsqu'elles se déchargent et perdent leur charge lentement lorsqu'elles sont stockées. 
 L'accumulateur au plomb-acide est également un type de batterie secondaire couramment utilisé dans les automobiles. Il est bon marché et capable de produire le courant élevé requis par les démarreurs d'automobiles. Les réactions d'une batterie au plomb sont : 
 <img alt="Eq5" src="/files/ftp_upload/11439/11439_Equation_5.png" style="text-align: center; height: 160px;" />
 Chaque cellule produit 2 V (Ecellule ~ 2 V), de sorte que six cellules sont connectées en série pour produire une batterie de voiture de 12 V. Les batteries au plomb-acide sont lourdes et contiennent un électrolyte liquide caustique, H2SO4 (aq), mais demeurent souvent la batterie de choix en raison de leur forte densité de courant. Comme ces batteries contiennent une quantité importante de plomb, on doit s'en débarrasser de manière appropriée. 
 Piles à combustible
 Une pile à combustible est une cellule galvanique qui utilise des combustibles traditionnels, le plus souvent de l'hydrogène ou du méthane, qui sont alimentés en permanence dans la pile avec un oxydant. À l'intérieur de la cellule, le combustible et l'oxydant sont soumis à la même chimie redox que lorsqu'ils subissent une combustion, mais via une catalyse électrochimique qui est beaucoup plus efficace. Par exemple, une pile à hydrogène type utilise des électrodes en graphite intégrées à des catalyseurs à base de platine pour accélérer les réactions des deux demi-cellules : 
 <img alt="Eq6" src="/files/ftp_upload/11439/11439_Equation_6.png" style="text-align: center; height: 130px;" />
 Ces types de piles à combustible produisent généralement des tensions d'environ 1,23 V (Ecellule ~ 1,23 V). Par rapport à un moteur à combustion interne, le rendement énergétique d'une pile à combustible utilisant la même réaction d'oxydoréduction est généralement plus du double (~20 %–25 % pour un moteur contre ~50 %–75 % pour une pile à combustible). Les piles à hydrogène sont couramment utilisées dans les missions spatiales prolongées et des prototypes de véhicules personnels ont été mis au point. 
 Ce texte est adapté de <a href="https://openstax.org/books/chemistry-2e/pages/17-5-batteries-and-fuel-cells"> Openstax, Chimie 2e, Section 17.5 : Batteries et piles à combustible. </a>

Batteries et piles à combustible

Une batterie est une pile galvanique qui est utilisée comme source d’énergie électrique pour des applications spécifiques. Les batteries modernes existent sous une multitude de formes pour ...

Education

Enseignement

JoVE Core

Chemistry

Chimie

Electrochemistry

Électrochimie

KEY TERMS AND CONCEPTS

TERMES ET CONCEPTS CLÉS

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 Chimie anime les concepts de chimie générale en utilisant des leçons vidéo concises et faciles à comprendre. De plus, nos vidéos de scientifiques à l'action présentent des expériences de recherche, classiques ou insolites, effectuées dans des laboratoires modernes du monde entier.

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

Description

Transcript

Tags

More videos by Standards