Why can t the energy of an activated molecule be transferred to an ordinary molecule? 5

Brief introduction. Molecules with energies above a certain threshold (low limit energy) are called activated molecules. Molecules with energies lower than this value are called inactive molecules or ordinary molecules.

In the process of movement and collision of molecules, energy exchange between molecules constantly occurs, so that the energy of each molecule is changing rapidly. As a result, even molecules of the same type can vary greatly in energy. This difference in energy separates the molecule into activated and non-activated molecules.

2] Activated and non-activated molecules are not set in stone. Due to molecular collision, some activated molecules will lose energy and become inactive molecules; Non-activated molecules may gain energy from the collision and become activated molecules. However, at a certain temperature, the number of activated molecules (or the percentage of activated molecules) is constant.

The energy of the activated molecule is higher than that of the ordinary molecule** than the collision kinetic energy of the molecule. Different molecules in the same system require different amounts of energy to be activated, so when one molecule is activated, another molecule may not be activated.

Mechanism of reaction. At the same temperature, the energy of molecules is not exactly the same, and some molecules have energy higher than the average energy of molecules, which is called activated molecules. It is the activated molecule that can have an effective collision, but the activated molecule does not necessarily have an effective collision.

It is not any direct interaction between the molecules of the reactants that can react, only the direct interaction between those molecules with a fairly high energy can react. At a certain temperature, the number of activated molecules in a reaction is determined by the activation energy EA of the reaction. According to Boltzmann's law of energy distribution, the fraction of the total number of molecules with energy greater than EA can be estimated by E-EA RT.

The number (or concentration) of activated molecules is an important factor in determining the rate of a chemical reaction. For a given chemical reaction, when the temperature (t) increases, the value of E-EA RT increases, the proportion of activated molecules increases, and the reaction rate increases. The use of catalysts can reduce the activation energy of the reaction, so that the reactant molecules with average energy can become activated molecules as long as they absorb less energy, which is conducive to increasing the chemical reaction rate.

The molecule must have enough energy to turn into an activated molecule for a reaction. The ways to increase the activation of molecules are:

1. Increase the concentration, because the percentage of activated molecules in the total number of molecules at a certain temperature is fixed;

2. Increase the temperature and increase the molecular energy;

3. Use catalyst to reduce the energy standard of the reaction.

An activated molecule is a molecule whose energy (referring to kinetic energy) is large enough to break a chemical bond when it collides with each other. For a certain molecule to undergo a certain reaction, the minimum energy of the activated molecule is a fixed value, which depends on the strength of the chemical bond and has nothing to do with the actual energy of the molecule. Molecules with energy above this minimum are activated molecules, and those below it are not activated molecules.

The average energy (kinetic energy) of a molecule is determined by temperature. The higher the temperature, the higher the percentage of molecules with energy exceeding the above minimum value (i.e., the number of activated molecules). The so-called ordinary molecule is a molecule with average energy, and the energy of a molecule exceeding the average energy does not necessarily cause chemical bond breakage (and it does not necessarily mean that it can't, that is to say, the energy of the activated molecule has nothing to do with the average energy of Pingxiao).

Vice versa. When considering this question, it is important to understand what is an activated molecule and what is an ordinary molecule. An effective collision can occur, and the molecule that initiates the break of the chemical bond is the activated masking molecule (the minimum energy required to initiate the break of the chemical bond depends on the bond energy, the greater the bond energy, the stronger the bond, and the greater kinetic energy must be provided to the colliding molecule in order to break in the collision).An ordinary molecule is a molecule with an average energy, and the average energy (kinetic energy) is determined by temperature.

There is no necessary connection between the activated molecule and the average energy of the molecule. Ordinary molecules can also be activated molecules (molecules with average energy can also cause bond breaks), but this can be misleading. Because in different contexts, the meaning of ordinary molecule can also refer to the molecule that is opposed to the activated molecule, and the energy is not enough to cause bond breakage (i.e., inactivated molecule).

This definition of ordinary molecules is personally considered inappropriate and easy to misunderstand, especially for beginners, and it is recommended that landlords do not adopt this definition.

The ordinary molecule in your textbook is the former meaning.

Feel free to keep us asking.

By the way, the understanding of activators on the first floor is wrong, and if it happens to be correct, it contradicts the statement of your textbook.

The statements in it are contradictory. are not professionals.

Relationship: The definition of "activator" is not very clear at this point. If it is considered to be a molecule with an energy higher than the activation energy, then the activation molecule increases exponentially as the activation energy decreases.

Because the energy of the molecule satisfies the Boltzmann distribution, which is an exponential distribution.

For example, to prepare copper oxide from copper sulfate, the first step is to react with copper sulfate and sodium hydroxide, and the second step is to heat and decompose copper hydroxide to prepare copper oxide. The first step is a metathesis reaction, the activation energy is very low, the speed is very fast, and the reaction is completed immediately.

But the second step is a decomposition reaction, the activation energy is high, and it needs to be calcined at high temperature to complete the reaction, so the total activation energy of this reaction is the activation energy of copper hydroxide heating and decomposition.

Bud. Activation energy is a chemical term, also known as threshold energy. The term was introduced by Arrhenius in 1889 to define the energy barriers that need to be overcome for a chemical reaction to occur.

Activation energy can be used to express the minimum amount of energy required for a chemical reaction to occur. The activation energy of a reaction is usually expressed as Ea in kilojoules per mole (kj mol). Activation energy represents the height of a potential barrier (sometimes called an energy barrier).

The magnitude of the activation energy can reflect the ease with which the chemical reaction occurs.

The above content is implicitly referenced: Encyclopedia - Reaction Activation Energy.

No, brother, right! For one reaction, the catalyst reduces the amount of energy required to activate the molecule. A molecule whose energy is just not enough to become an active molecule without a catalyst is higher than a molecule that is activated after adding a catalyst.

Not necessarily. In different reactions.

An activated molecule may have a lower energy than a normal molecule.

At the same temperature, the energy of the molecules is not exactly the same, and some molecules have higher energy than the molecules, which are called activated molecules.

Note: Average energy. Not the "highest energy".

You still don't understand what LS is talking about...

The higher the energy, the higher the ratio of the activated energy molecules to the total number of molecules, but not all of them are converted into activated molecules.

The kinetic energy of a molecule is <> of the Maxwell-Boltzmann distribution (figure below).

This is the velocity distribution of 10 6 oxygen molecules at temperatures of -100 °C, 20 °C and 600 °C. The higher the temperature, the higher the average kinetic energy of the molecules, and as you can see, the peak occurs at a higher velocity (or higher energy), but there are always some molecules that have only low non-activated energy.

1) As can be seen from the figure, when there is no enzyme catalysis, the activation energy required for the occurrence of chemical anti-aging is higher, and when there is enzyme catalysis, the activation energy required for the occurrence of chemical marketing and wisdom reaction is lower, so the essence of enzyme catalysis is to reduce the activation energy of chemical reaction

2) The chemical nature of enzymes is protein or RNA, and enzymes can work both inside and outside the cell, so the answer is: 1) Higher Lower Enzyme Reduced Activation Energy Reduces Activation Energy of Chemical Reactions.

2) Protein or RNA intracellular or extracellular.