Question

For many reactions, it is found that a large number of colliding molecules have energy more than threshold value,yet the rate of the reaction is slow. What might be the reason?

Answer 1

Answer:

Hey mate here is your answer.//

Explanation:

The main reason behind the reaction to be slow even after a large number of colliding molecules have energy more than threshold energy for a reaction, is because of the improper alignment of the molecules which are colliding.

The theory of Collision considers the following assumptions:

The chemical reaction rate is directly proportional to the number of collisions which the reactant molecules undergo in a given time.

                 Reaction Rate = (number of Collisions) / Time

The collision should be in an alignment which facilitates contact between the atoms which are favorable to bond together into a product.

The collision must occur with adequate energy, that should be more than the threshold energy, to permit mutual penetration of the reacting species’ valence shells which allows the electrons to realign and create new bonds.

According to the Collision theory most of the rate of reaction increases, as concentrations increases. As the number of molecules per unit of volume increases, with the increase in concentration of the reacting substance, the chances for collision between molecules increases. With an increase in collision, reaction rate also increases, under the assumption that the energy of collisions is adequate.  

Hope t helps you.//✔✔✔

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