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A reaction is designated as exergonic when it releases energy, typically in the form of free energy, during the process. This is characterized by a negative change in Gibbs free energy (ΔG < 0), indicating that the products have less free energy than the reactants. In contrast, an endergonic reaction requires an input of energy, resulting in a positive change in Gibbs free energy (ΔG > 0).
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Is movement an exergonic reaction?
Movement is not considered an exergonic reaction. Exergonic reactions typically refer to chemical reactions that release energy, while movement in living organisms is driven by processes such as muscle contraction and nerve impulses rather than by a specific chemical reaction.
How can an Endergonic reaction not be Endothermic?
An endergonic reaction is characterized by a positive change in Gibbs free energy, meaning it requires energy input to proceed. However, this does not necessarily mean it is endothermic, as endothermic reactions specifically absorb heat from their surroundings. An endergonic reaction could be driven by other forms of energy, such as light or electrical energy, rather than heat. Thus, while all endothermic reactions can be endergonic, not all endergonic reactions are endothermic.
Is heat the only possible result of exergonic reaction?
No, heat is not the only possible result of an exergonic reaction. While exergonic reactions release energy, this energy can be transformed into different forms, such as light or mechanical work, depending on the specific reaction and conditions. For example, in biological systems, the energy released during cellular respiration can be used to drive ATP synthesis rather than simply being released as heat.
Why does the total amount of energy does not decrease in an exergonic chemical reaction?
In an exergonic chemical reaction, the total amount of energy does not decrease because energy is conserved according to the law of thermodynamics. Instead, the reaction releases energy to the surroundings, usually in the form of heat or light, while the total energy in the system and surroundings remains constant. The energy released comes from the difference in potential energy between the reactants and products, not from a loss of total energy. Thus, the total energy is redistributed rather than diminished.
What determines how much energy is available in a molecule?
This is related to the Gibbs free energy: G = H —TS (where, H is the enthalpy, T is the absolute temperature, and S is the entropy), that is the required indicator of spontaneity for constant temperature and pressure processes. For systems that can only do pressure - volume work (w' = 0), Gibbs free energy equation can be expressed as: DG = DH — TDS = qp — TDS (where, qp is the heat transferred at constant pressure). Now, a spontaneous process is that one with negative DG value and is said to be "exergonic" and it can be utilized to do work. A process that is not spontaneous, that one with positive DG value is called "endergonic" and it must be driven by the input of free energy. Those processes that are at equilibrium (when the forward and the backward reactions are exactly balanced) are characterized by a DG = 0. From above considerations, the endergonic processes that maintain the living state are driven by the exergonic reactions of nutrient oxidation. Living organisms are not at equilibrium. Rather, they require a continuous influx of free energy to maintain order in a universe bent of maximizing disorder. They do so by coupling the exergonic processes required to maintain the living state such as the performance of mechanical work, the active transport of molecules against concentration gradients, and the biosynthesis of complex molecules. The key is to know "how much free energy carry a particular molecule" in order to carry out a work. This can be achieved measuring the "free energy" of a given intermediate molecule whose exergonic consumption drives endergonic processes. In other words, to determine how much "energy" carries a particular molecule, we have to measure its DG value.
Is the Calvin cycle endergonic or exergonic?
Yes, the Calvin cycle is endergonic because it uses ATP molecules rather than creates them.
Is movement an exergonic reaction?
Movement is not considered an exergonic reaction. Exergonic reactions typically refer to chemical reactions that release energy, while movement in living organisms is driven by processes such as muscle contraction and nerve impulses rather than by a specific chemical reaction.
How can an Endergonic reaction not be Endothermic?
An endergonic reaction is characterized by a positive change in Gibbs free energy, meaning it requires energy input to proceed. However, this does not necessarily mean it is endothermic, as endothermic reactions specifically absorb heat from their surroundings. An endergonic reaction could be driven by other forms of energy, such as light or electrical energy, rather than heat. Thus, while all endothermic reactions can be endergonic, not all endergonic reactions are endothermic.
Why is photosynthesis considered an endergonic reaction in an isolated plant?
Photosynthesis is considered an endergonic reaction because it requires energy input from sunlight to convert carbon dioxide and water into glucose and oxygen. This process is endergonic because it absorbs energy rather than releasing it. In an isolated plant, the plant must obtain this energy from sunlight to drive the photosynthetic reaction.
Is heat the only possible result of exergonic reaction?
No, heat is not the only possible result of an exergonic reaction. While exergonic reactions release energy, this energy can be transformed into different forms, such as light or mechanical work, depending on the specific reaction and conditions. For example, in biological systems, the energy released during cellular respiration can be used to drive ATP synthesis rather than simply being released as heat.
Do formation and breaking bonds involve taking in or giving off energy?
Yes. That's rather less informative than it might be had the question been worded a bit more exclusively. The formation of bonds is exergonic, while the breaking of bonds is endergonic.
Why does the total amount of energy does not decrease in an exergonic chemical reaction?
In an exergonic chemical reaction, the total amount of energy does not decrease because energy is conserved according to the law of thermodynamics. Instead, the reaction releases energy to the surroundings, usually in the form of heat or light, while the total energy in the system and surroundings remains constant. The energy released comes from the difference in potential energy between the reactants and products, not from a loss of total energy. Thus, the total energy is redistributed rather than diminished.
Is photosynthesis an exothermic or endothermic reaction?
Yes photosynthesis is a endergonic process i.e. energy-requiring process.
What determines how much energy is available in a molecule?
This is related to the Gibbs free energy: G = H —TS (where, H is the enthalpy, T is the absolute temperature, and S is the entropy), that is the required indicator of spontaneity for constant temperature and pressure processes. For systems that can only do pressure - volume work (w' = 0), Gibbs free energy equation can be expressed as: DG = DH — TDS = qp — TDS (where, qp is the heat transferred at constant pressure). Now, a spontaneous process is that one with negative DG value and is said to be "exergonic" and it can be utilized to do work. A process that is not spontaneous, that one with positive DG value is called "endergonic" and it must be driven by the input of free energy. Those processes that are at equilibrium (when the forward and the backward reactions are exactly balanced) are characterized by a DG = 0. From above considerations, the endergonic processes that maintain the living state are driven by the exergonic reactions of nutrient oxidation. Living organisms are not at equilibrium. Rather, they require a continuous influx of free energy to maintain order in a universe bent of maximizing disorder. They do so by coupling the exergonic processes required to maintain the living state such as the performance of mechanical work, the active transport of molecules against concentration gradients, and the biosynthesis of complex molecules. The key is to know "how much free energy carry a particular molecule" in order to carry out a work. This can be achieved measuring the "free energy" of a given intermediate molecule whose exergonic consumption drives endergonic processes. In other words, to determine how much "energy" carries a particular molecule, we have to measure its DG value.
What type of reaction is NaCI?
NaCl is not a reaction, but rather a compound.
What is the meaning of word catalyst?
A catalyst speeds up a reaction by lowering the activation energy of the reaction. It is not consumed by the reaction, but rather it leaves the reaction unchanged.
What is some evidence that suggests that a nuclear reaction is occurring rather than a chemical reaction?
Beacause they are very alike & Then They Get Wild
