2.what do you called the minimum energy required for a reaction to happen?, 3.what do you called the collision between two particles that causes a chemical reaction to happen?, 4.based on the illustration, how do you know the first reaction is not a successful collision?



2.what do you called the minimum energy required for a reaction to happen?


3.what do you called the collision between two particles that causes a chemical reaction to happen?
4.based on the illustration, how do you know the first reaction is not a successful collision?​

Answer:

Activation energy

Successful collision or an effective collision.

Activation Energy and Temperature

Explanation:

Activation energy is the minimum energy required to cause a process (such as a chemical reaction) to occur.

Molecules must collide with sufficient energy, known as the activation energy, so that chemical bonds can break. Molecules must collide with the proper orientation. A collision that meets these two criteria, and that results in a chemical reaction, is known as a successful collision or an effective collision.

In order for a collision to be successful by resulting in a chemical reaction, A and B must collide with sufficient energy to break chemical bonds. This is because in any chemical reaction, chemical bonds in the reactants are broken, and new bonds in the products are formed.



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