Regarding the question of activating molecules, what is the activation energy related to molecules?

The process of chemical reaction can be summarized in a diagram, sorry I can't pass the diagram yet, just make it live, imagine.

It's like the cut-off score for admission. The score line is 460, and if you take the 470 test, you can get in, but if you take the 450 test, you can't go in. Adding a positive catalyst is equivalent to lowering the score line, and the score line of 440 and the score line of 450 can also be entered.

Of course, there are more people who can get into that school. (The positive catalyst can increase the percentage of activated molecules) and the ability of people has not changed, so it is said that the average energy of the molecule has not been reduced.

I don't know if you can understand me when I explain it like this. Sweat.

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 has an effective collision, but the activated molecule does not necessarily have an effective collision. At a certain temperature, the number of activated molecules in a reaction is determined by the activation energy EA of the reaction.

Activation energy refers to the minimum amount of energy required by the reactant molecule to reach the activated molecule in a chemical reaction. An effective collision is possible only when the energy of the colliding molecule equals or exceeds a certain energy ec (which can be called critical energy). Therefore, when the catalyst is added, the reaction pathway is changed and the activation energy of the reaction is reduced.

When the activation energy is reduced, the activated molecules increase and the percentage increases, so the reaction speed is increased, of course, for the positive catalyst.

For example, without a catalyst, 100 can react.

When using a catalyst, the reaction can be carried out with 50 of the "50".

So it's equivalent to a lot of activated molecules.

The catalyst does not provide the energy required for the reaction, so there is no increase in energy, etc., he participates in the reaction, but in the end it changes back, and he indirectly "makes" the reactants, unstable substances, to achieve the purpose, which is equivalent to reducing the energy and equivalent to activating more molecules.

Relationship: The definition of "activated molecule" is not very clear right now. If you think of 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 reference: Encyclopedia - Reaction Activation Energy.

The energy required for a molecule to change from a normal state to an active state prone to chemical reactions is called.

Activation energy. Activated molecules, at the same temperature, the energy of the molecules is not exactly the same, and the energy of some molecules is higher than the average energy of the molecule, 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.

Increase the concentration of reactants per unit volume.

The number of internally activated molecules increases, but the percentage.

unchanged, so the scum is not chosen;

Increasing the temperature can increase the number of activated molecules and the percentage of activated molecules in the reactants at the same time, so it is selected;

When the pressure increases, the number of activated molecules per unit volume increases, but the percentage remains unchanged, so it is not selected.

When the product is removed, the concentration decreases, and the number of activated molecules and the number of beams in the unit volume decreases, so it is not selected;

The addition of catalyst can increase the number of activated molecules and the percentage of activated molecules in the reactant at the same time, so it is selected;

Therefore, a

There are no examples of this. It's just a model.

For molecules to react, they must collide. But not all collisions can react, which is understandable, so the part of the collision that will react is called an effective collision.

One of the conditions for an effective collision is that both the colliding molecules have sufficient energy. We call these molecules with sufficient energy as activated molecules. So, why don't all collisions work?

It's because those molecules don't have enough energy, it's like they can't hit a spark and can't ignite.

So the more activated molecules, the more effective the collision will be.

The difference between an activated molecule and an ordinary molecule is energy. The energy difference between the two is the activation energy. Obviously, the smaller the activation energy, the closer the two are, and the more naturally activated molecules there are.

Activation energy is the difference between the average energy of an activated molecule and the average energy of an ordinary molecule. Therefore, the higher the activation energy, the fewer molecules that can reach high energy, and the less chance of effective collision. The harder it is to react!

Hydrogen and oxygen do not react at room temperature, but react when heated or ignited, which provides activation energy to the reactants to carry out the reaction.

Activation energy is the amount of energy required for the reaction The energy of the molecule is large and small The activated molecule is the molecule that conforms to the activation energy Generally, the energy is relatively high, that is, the speed is large, the activation energy is like the height of the mountain, the higher the mountain, the more difficult it is to climb Reducing the activation energy is equivalent to making a tunnel under the mountain It doesn't take so much energy to pass through The positive catalyst can generally be understood in this way The reaction between molecules needs to collide It is necessary to have the right direction and enough energy The more molecules with energy, the smaller the energy required (that is, the activation energy) The more collisions are in the right direction, the more violent the reaction will be.

Activation energy. It refers to the minimum amount of energy required by the reactant molecule to reach the activated molecule in a chemical reaction. The activation energy is not equal to the total bond energy of the reactants.

Please explain.

It's good to have it.

The magnitude of the activation energy itself is determined by the material structure. Right. So.

How does the catalyst change the amount of activation energy?

The catalyst can change the reaction process, under normal circumstances, the catalyst participates in the reaction, has a relatively small activation energy, and then releases the catalyst at a certain stage, and the new process reaction is relatively easy to carry out.

Activated molecules are formed by ordinary molecules after absorbing a certain amount of energy.

So can it be considered so?

What about a molecule that breaks its bonds to absorb energy?

In what form do activated molecules exist?

Molecular bond breaking absorbs energy, and activated molecules have slightly higher energy than other molecules, and the speed of movement is relatively fast.

And also. After activating the molecule reaction.

In what way is the activation energy converted?

It's heat. If yes.

Thermal energy. Then the heat of reaction obtained by the test.

Isn't that accurate?

Or will it be far away?

The average energy of the molecule is constant, the energy of the activated molecule is high, and the energy of other molecules is low, which will not affect the heat of reaction.

The higher the activation energy, the more difficult it is to activate the molecular cluster" is wrong with the phrase "the more difficult it is for the molecule to activate".

It is correct to say that "the higher the activation energy, the easier it is for the molecule to activate".

Isn't it that the higher the activation energy, the higher the energy required for the molecule to become active, how is it that the more quietly and solemnly it is easy to activate the ruler?

The higher the activation energy, the less energy is required for the molecule to become active, and the easier it is for the molecule to activate. (Just omit a sentence, you don't understand it).

Read more textbooks.