Name: cell reactions that release or store energy
Uploaded: 2023-04-30T10:41:14.000Z
Duration: 1 min 27 s
Channel: JoVE

K12 Standards

Tennessee Academic Standards

High School

Chemistry

Energy

CHEM1.PS3.3

endergonic-and-exergonic-reactions-in-the-cell

Endergonic and Exergonic Reactions in the Cell

Si la variation d’énergie libre est inférieure à zéro, le processus est spontané et s’appelle une réaction exergonique. En revanche, si la variation d’énergie libre est supérieure à zéro, le processus n’est pas spontané et la réaction est endergonique.
Pour comparer les changements d’énergie de différentes réactions, le changement d’énergie libre est généralement signalé sous un ensemble standard de conditions écrites comme suit : ΔG0.
L’hydratation du fumarate en malate en présence de fumarase est une réaction exergonique car la variation standard de l’énergie libre pendant le processus est de −3,8 kJ/mol.
Pour que des réactions endergoniques se produisent, de l’énergie doit être ajoutée au système. Dans les cellules, les réactions endergoniques sont couplées à des réactions exergoniques.
Par exemple, la conversion endergonique du glucose en glucose-6-phosphate a une variation d’énergie libre standard de 13,8 kJ/mol, et l’hydrolyse exergonique de l’ATP a une variation d’énergie libre standard de -30,5 kJ/mol.
Ces réactions sont couplées à l’intérieur de la cellule, et l’ensemble du processus est exergonique, avec une variation d’énergie libre standard de -16,7 kJ/mol, soit un total de l’énergie libre standard des deux procédés.

réactions endergoniques et exergoniques dans la cellule

Si de l'énergie est libérée lors d'une réaction chimique, la valeur résultante sera un nombre négatif. En d'autres termes, les réactions qui libèrent de l'énergie ont un ∆G < 0. Un ∆G négatif signifie également que les produits de la réaction ont moins d'énergie libre que les réactifs car ils ont dégagé une certaine énergie libre pendant la réaction. Les scientifiques appellent réactions exergoniques les réactions présentant un ∆G négatif et qui libèrent par conséquent de l'énergie libre. Exergonique signifie que l’énergie quitte le système. Nous appelons également ces réactions des réactions spontanées, car elles peuvent se produire sans ajouter d’énergie dans le système. Comprendre quelles réactions chimiques sont spontanées et libèrent de l’énergie libre est extrêmement utile pour les biologistes, car ces réactions peuvent être exploitées pour effectuer des travaux à l’intérieur de la cellule. Contrairement à l’usage courant du terme, une réaction spontanée n’est pas une réaction qui se produit soudainement ou rapidement. La rouille du fer est un exemple de réaction spontanée qui se produit lentement, petit à petit, au fil du temps.

Si une réaction chimique nécessite un apport d’énergie, alors le ∆G de cette réaction sera une valeur positive. Dans ce cas, les produits ont plus d’énergie libre que les réactifs. Ainsi, nous pouvons considérer les produits des réactions comme des molécules stockant de l’énergie. Nous appelons ces réactions chimiques des réactions endergoniques et elles ne sont pas spontanées. Une réaction endergonique ne se produira pas d’elle-même sans ajout d’énergie libre.

Par exemple, la construction de molécules complexes, comme les sucres, à partir de molécules plus simples est un processus anabolique qui nécessite de l’énergie. Les réactions chimiques impliquées dans les processus anabolisants sont donc des réactions endergoniques. Alternativement, le processus catabolique consistant à décomposer le sucre en molécules plus simples libère de l'énergie dans une série de réactions exergoniques.

Ce texte est adapté d'Openstax, Biologie 2e,​ <a href="https://openstax.org/books/biology-2e/pages/6-2-potential-kinetic-free-and-activation-energy">Section 6.2: </a><a href="https://openstax.org/books/biology-2e/pages/6-2-potential-kinetic-free-and-activation-energy-of-thermodynamics">Potential, Kinetic, Free, and Activation Energy</a>.

Réactions Endergoniques et Exergoniques dans La Cellule

Si de l’énergie est libérée lors d’une réaction chimique, la valeur résultante sera un nombre négatif. En d’autres termes, les réactions qui libèrent de l’énergie ont ...

Education

Enseignement

JoVE Core

Cell Biology

Biologie cellulaire

Unit 1

Unité 1

Energy and Catalysis

Énergie et catalyse

KEY TERMS AND CONCEPTS

TERMES ET CONCEPTS CLÉS

cell reactions that release or store energy

Cell reactions can either release energy or store it for later use. In chemistry, this difference is described by the value of ΔG, or free energy change. When energy is released during a reaction, ΔG is negative. The products then have less free energy than the reactants because some free energy has been given off.

Reactions with a negative ΔG are called exergonic reactions. Exergonic means energy is leaving the system. These reactions are also called spontaneous reactions because they can happen without adding energy to the system. In biology, this matters because cells can use these reactions to do work.

The word spontaneous does not mean fast. A spontaneous reaction can still happen slowly over time. Rusting iron is a good example. It is spontaneous, but it occurs little by little.

If a reaction needs an energy input, its ΔG is positive. In that case, the products have more free energy than the reactants. These products can be thought of as energy-storing molecules. Such reactions are called endergonic reactions, and they are non-spontaneous. They do not occur on their own unless free energy is added.

Cells use both kinds of reactions in metabolism. Building complex molecules, such as sugars, from simpler ones is an anabolic process. It requires energy, so the reactions are endergonic. Breaking sugar down into simpler molecules is a catabolic process. This breakdown releases energy in a series of exergonic reactions.

Cell Reactions That Release or Store Energy

cell-reactions-that-release-or-store-energy

the first law of thermodynamics

Energy Changes in Cells and Matter

The first law of thermodynamics describes how energy changes form in the universe. The total amount of energy stays constant. Energy can move from one place to another or change into a different form, but it cannot be created or destroyed. These energy changes happen in everyday life. A light bulb changes electrical energy into light energy. A gas stove changes chemical energy in natural gas into heat energy. Plants also carry out a major energy transformation when they convert sunlight energy...

the second law of thermodynamics

Entropy and Spontaneous Change

Entropy helps predict whether a process will happen on its own. Entropy is a measure of randomness or disorder in a system. High entropy means high disorder and low energy. A student’s bedroom is a simple example. If no work is done, the room becomes messy over time. That messy state is highly disordered and has high entropy. To make the room clean again, energy must be added as the student puts things away. That organized state has low entropy. Processes that increase the entropy of the...

enthalpy within the cell

Cellular Enthalpy and Energy Changes

Cellular enthalpy describes how heat and energy change during chemical and physical processes. Enthalpy is written as H and is defined as the sum of a system’s internal energy, U, and the product of pressure and volume, PV. It is a state function, which means its value depends on the state of the system, not the path taken. Scientists cannot measure the enthalpy of a single substance directly. They can determine enthalpy changes, or ΔH, for a process instead. For reactions or changes that...

entropy within the cell

Cell Energy Loss and Entropy

Cell energy loss and entropy explain why living things need constant energy input. Cells obtain energy, transform it, and use it to do work, but these transfers are never completely efficient. In each transfer, some energy is lost in a form that cannot be used. In many cases, that lost energy is heat energy.

an introduction to free energy

Gibbs Free Energy and Reaction Work

Gibbs free energy describes the usable energy in a chemical reaction. It helps scientists compare how much energy different reactions release. This measurement is called Gibbs free energy, or G, after Josiah Willard Gibbs. The second law of thermodynamics explains why not all energy stays available for work. Some energy is lost in an unusable form, such as heat, and this loss increases entropy. Gibbs free energy is the energy left after that entropy loss is taken into account. Every chemical...

endergonic and exergonic reactions in the cell

Cell reactions can either release energy or store it for later use. In chemistry, this difference is described by the value of ΔG, or free energy change. When energy is released during a reaction, ΔG is negative. The products then have less free energy than the reactants because some free energy has been given off. Reactions with a negative ΔG are called exergonic reactions. Exergonic means energy is leaving the system. These reactions are also called spontaneous reactions because they can...

the equilibrium binding constant and binding strength

the-equilibrium-binding-constant-and-binding-strength

How Equilibrium Binding Constant Affects Binding

The equilibrium binding constant describes how strongly two molecules bind at equilibrium. It is a useful way to compare binding strength in molecular interactions. This topic focuses on how binding is measured and what the equilibrium binding constant means. A higher value indicates stronger binding, while a lower value indicates weaker binding. Understanding this constant helps explain how tightly molecules stay together under equilibrium conditions. The page also connects the binding...

free energy and equilibrium

Free Energy and Reaction Direction

Free energy and reaction direction are linked in chemical equilibrium. A free energy change, ΔG, shows the driving force for a process. When ΔG is negative, the process is driven forward. When ΔG is positive, the reverse direction is favored. When ΔG is zero, the forward and reverse driving forces are equal, and the system is at equilibrium. The reaction quotient, Q, helps show how close a system is to equilibrium. Q is the numerical value of the mass action expression for the system. It can...

non-equilibrium in the cell

Cells Stay Out of Equilibrium

Cells stay out of chemical equilibrium by constantly using energy and moving materials in and out. Chemical reactions in metabolism are often reversible. They can go in both directions. In one direction, they release energy to the surroundings. In the reverse direction, they absorb energy. The same idea applies to reactions that build and break down cell molecules. Proteins, for example, can be broken into individual amino acids, and amino acids can be used to build proteins again. In a closed...

oxidation and reduction of organic molecules

oxidation-and-reduction-of-organic-molecules

Electron Carriers in Cell Energy Transfer

Cell energy production depends on redox reactions, which are oxidation and reduction reactions that happen together. In oxidation, an electron is removed from an atom in a compound. In reduction, that same electron is added to another compound. Because these reactions usually occur as a pair, they are called redox reactions. When a molecule loses an electron, its potential energy goes down. The electron does not stay free in the cytoplasm. Instead, it moves to a second compound and reduces...

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Enzyme Function, Cofactors, and Inhibitors

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enzymes and activation energy

How Enzymes Lower Reaction Energy

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Graphing Enzyme Kinetics Data

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turnover number and catalytic efficiency

How Fast Enzymes Work in Digestion

Enzymes can work at very different speeds, and their turnover number shows how fast they convert substrate molecules into products. Turnover number is the maximum number of substrate molecules an enzyme can transform per unit time. For most enzymes, this value is between 1 and 1000 molecules per second. Some enzymes are especially fast. Catalase has the highest known turnover number and can convert up to 2.8×10^6 molecules of hydrogen peroxide into water and oxygen each second. Lysozyme has...

catalytically perfect enzymes

Diffusion-Controlled Enzymes and Reaction Speed

Catalytically perfect enzymes are enzymes that speed up biochemical reactions at very high rates. The idea was first proposed by W. J. Albery and J. R. Knowles in 1976. These enzymes have catalytic efficiency values of about 10^8 to 10^9 M^-1 s^-1 and are also called diffusion-controlled enzymes because diffusion of the substrate into the active site is the only rate-limiting step. Examples of catalytically perfect enzymes include triose phosphate isomerase, fumarase, and superoxide dismutase.

introduction to mechanisms of enzyme catalysis

introduction-to-mechanisms-of-enzyme-catalysis

How Enzymes Change Shape to Catalyze

Enzyme catalysis depends on how enzymes bind substrates and how the active site responds during the reaction. Scientists once described this process with a simple lock-and-key model, where the enzyme and substrate fit together in one instant. Research now supports induced fit, a more dynamic model in which binding causes a small change in the enzyme’s shape. That shift helps create an ideal match between the enzyme and the substrate’s transition state, which improves catalysis. The active site...

ligand binding and linkage

Ligand Binding and Allosteric Effects

Ligand binding and linkage describe how one molecule can affect another when it binds to a protein. In this topic, the focus is on how binding at one site can influence activity at a different site on the same protein. This idea is important for understanding protein function in high school biology. It helps explain why some proteins respond more strongly after a ligand attaches. The transcript centers on the connection between ligand binding and linkage, which is a key concept in molecular...

cooperative allosteric transitions

How Proteins Shift Shape Together

Proteins can change shape in a coordinated way during allosteric transitions. In a cooperative transition, one part of the protein affects another part, so the change spreads through the molecule. These shape changes help proteins switch between different states. The shift can influence how the protein works and how it responds to other molecules. Cooperative allosteric transitions are an important idea in protein function. They explain how a small change at one site can lead to a larger...

ribozymes

Catalytic RNA: Ribozymes in Action

Ribozymes are RNA molecules that can act as enzymes. They help speed up specific chemical reactions without being protein enzymes. This makes them an important example of RNA with more than one job in the cell. Some ribozymes can cut RNA molecules, and others can join them together. This shows that RNA can do catalytic work as well as carry genetic information. Ribozymes are a key part of how scientists think about the many roles of RNA in biology. One well-known ribozyme is ribonuclease P,...

atp energy storage and release

ATP Powers Cellular Transport and Reactions

ATP powers cellular transport and many reactions by transferring energy through phosphorylation. ATP is a highly unstable molecule. If it is not used quickly, it breaks down into ADP and inorganic phosphate, and the released energy is lost as heat. Cells use ATP through energy coupling. This means the exergonic reaction of ATP hydrolysis is linked to an endergonic reaction so the reaction can move forward. One major example is the sodium-potassium pump, a transmembrane ion pump that is vital...

atp and macromolecule synthesis

ATP in Building Cell Macromolecules

ATP helps cells build biological macromolecules. These organic compounds are mainly made of carbon atoms bonded to hydrogen, oxygen, nitrogen, and small amounts of other elements. The four major classes of biological macromolecules are carbohydrates, lipids, proteins, and nucleic acids. Most macromolecules start as small subunits called monomers. Cells join monomers with covalent bonds to make larger molecules called polymers. This building process needs energy, so cells depend on ATP, the...

coupled reactions

ATP Powers Cellular Work

ATP powers many kinds of cellular work by coupling energy-releasing reactions to energy-requiring ones. Some reactions happen on their own and release energy. Others need an energy input to move forward. Cells link these reactions so important processes can still occur. Adenosine triphosphate, or ATP, stores energy that cells can use quickly. ATP hydrolysis is the breaking of ATP, and it releases energy. Cells often use that released energy to drive endergonic reactions, which are reactions...

key terms and concepts

Learn how ΔG shows whether a cell reaction is exergonic or endergonic, why spontaneous does not mean fast, and how cells use these reactions.

Cell Reactions That Release or Store Energy | JoVE K12

cell biology

JoVE Core Biologie cellulaire illustre les processus cellulaires complexes dans des leçons vidéos complètes mais faciles à comprendre. Cette collection se concentre sur les composants et fonctions essentiels de la cellule ; cela inclut les organelles et les membranes ainsi que le transport et le métabolisme énergétique cellulaire. Elle est complétée par nos vidéos de scientifiques à l'action qui démontrent l'application de la biologie cellulaire dans des expériences concrètes.

Minnesota Academic Standards in Science

9-12

3.1.1 9C.2.2.1.1

Next Generation Science Standards

Life Science

from-molecules-to-organisms-structures-and-processes

From Molecules to Organisms: Structures and Processes

HS-LS1-7

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

South Carolina College and Career Ready Science Standards

C-PS3-4

Physics

P-PS3-3

Quantifying Heat

Thermal Energy&#160;

Microscopically, thermal energy is the kinetic energy associated with the random motion of atoms and molecules. Temperature is a ...

Temperature and Thermal Equilibrium

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Types of Kinetic Energy

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Kinetic Molecular Theory: Molecular Velocities, Temperature, and Kinetic Energy

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Constant Pressure Calorimetry

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Contrast the concepts of temperature and heat flow in macroscopic and microscopic terms. Understand that thermal energy is a form of energy and temperature is a measure of average kinetic energy of a particle. EXPLANATION: Students have been exposed to the types of energy (potential, kinetic, thermal, and chemical) and energy transfer (working, heating, and radiating) in the sixth grade. At that time, students classified energy types in systems and transformations. The focus in Chemistry 1 should be on understanding that measuring the temperature of a system is a way to quantify the thermal energy (average kinetic energy) of the particles in that system. Heating is a mechanism that transfers energy to or from a system. Students should also explore absolute vs relative scales of temperature mechanisms. Students should recognize that energy will always flow from objects with greater thermal energy to areas with lesser thermal energy, but rates of energy flow are a property of the materials being heated. The degree to which the temperature changes as an object is also a physical property of a material. Activities may include collecting or analyzing pressure vs temperature data, then considering why a graph of collected data does not pass through the origin. (Heat capacity and conductivity will only be assessed qualitatively.)

CHEM1.PS3.1

Heating and Cooling Curves

When a substance&#8212;isolated from its environment&#8212;is subjected to heat changes, corresponding changes in temperature and phase of the substance ...

Calorimetry

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Heat Exchanger Analysis

Source: Alexander S Rattner and Christopher J Greer; Department of Mechanical and Nuclear Engineering, The Pennsylvania State University, University Park, ...

Differential Scanning Calorimetry

Source: Danielle N. Beatty and Taylor D. Sparks, Department of Materials Science and Engineering, The University of Utah, Salt Lake City, UT
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Constant Volume Calorimetry

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Conservation of Energy

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Draw and interpret heating and cooling curves and phase diagrams. Analyze the energy changes involved in calorimetry by using the law of conservation of energy quantitatively (use of $q=mc\Delta T)$ and qualitatively. EXPLANATION: This is one of two standards where students are to investigate changes in a specific types of energy: In this case, thermal energy and phase energy. Starting as early as kindergarten, students are introduced to solid and liquid phases of matter. By third grade, students are considering the particulate nature of matter to discuss physical properties of the different phases. In fifth grade, students discuss phase changes from the perspective of the arrangement of particles. Chemistry 1 is the first time that students make a connection between phase changes and energy changes. Students commonly struggle with the idea that substances can be heated, but that heating does not always result in a change in temperature. Models of phase energies associated with the arrangement of particles aid in dispelling these misconceptions. Comparisons should identify similarities in energies in solids and liquids as compared to vastly different energy in gases. Discussions of heat of fusion/vaporization and calculations to enrich these discussions are appropriate. Finally, students should be able to quantify relationships in which heating creates a change in the thermal energy of a sample. Activities may include determining energy released when an object is burned to change the temperature of a substance in a closed system. (Note that this standard is limited to calculations of energy associated with changes in thermal energy, and not energies associated with phase transformations.)

CHEM1.PS3.2

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 ...

energy-diagrams-transition-states-and-intermediates

Energy Diagrams, Transition States, and Intermediates

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Energy Basics

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Chemical changes and their accompanying ...

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Thermochemical Equations

For a chemical reaction (the system) carried out at constant pressure &ndash; with the only work done caused by expansion or contraction &ndash; the ...

Activation Energy

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Bond Energies and Bond Lengths

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Introduction to Chemical Reactions

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bond-dissociation-energy-and-activation-energy

Bond Dissociation Energy and Activation Energy

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Distinguish between endothermic and exothermic reaction by constructing potential energy diagrams and explain the differences between the two using chemical terms (e.g. activation energy). Recognize when energy is absorbed or given off depending on the bonds formed and bonds broken. EXPLANATION: This is one of two standards where students are to investigate changes in a specific type of energy: In this case, chemical energy. Students should recognize that the formation of bonds releases energy, while the breaking of bonds is endothermic. Synthesis reactions to form metal oxides can provide observations if carried out taking proper precautions. Clear changes to masses and physical properties provide evidence of a reaction. (Specific discussions of enthalpy of formation are beyond the scope of this standard, but the topic may be useful for enrichment discussions about reactions where bonds are both broken and formed.)

Conservation of Energy: Application

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Conservation of Energy Approach to System Analysis

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First Law of Thermodynamics

Energy Conservation

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Conservation of Mechanical Energy

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Energy and Work

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Conservative Forces

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Non-conservative Forces

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Energy Diagrams - I

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Energy Diagrams - II

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Analyze energy changes to explain and defend the law of conservation of energy. EXPLANATION: Standards PS3.2 and PS3.3 identify the energy types most commonly associated with chemical reactions and build on sixth grade discussions of energy storage and transfer types. In Chemistry 1, students will synthesize an understanding of law of conservation of energy by being able to distinguish system from surroundings, and recognizing that tracking energy requires both the system and surrounding energies to be considered. Students can consider interactions such as a beverage warming/cooling, a refrigerator cooling food, the function of Freon in cooling systems, or a car's cooling system as examples where multiple systems interact.

CHEM1.PS3.4

Cell Reactions That Release or Store Energy

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