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Explain collision theory of reaction rate with an example.

Explain collision theory of reaction rate with an example.

Grade:upto college level

1 Answers

Sunil Kumar FP
askIITians Faculty 183 Points
7 years ago
For a reaction to occur, molecules must collide. The collision frequency describes how many times a particular molecule collides with others per unit of time.However, not all collisions result in a reaction. In order for molecules to react, a physical chemist named Svante Arrhenius explained,the colliding molecules must possess enough kinetic energy to overcome the repulsive and bonding forces of the reactants. The minimum amount of energy required for a chemical reaction to occur is known as the activation energy, denoted Ea.

The higher the Ea of a reaction, thesmaller the amount of energetic collisions present, and the slower the reaction.Energetic collisions are collisions between molecules with enough kinetic energy to cause the reaction to occur. Not all collisions are energetic collisions because they do not provide the necessary amount of Ea, so not all collisions lead to reactions and product formation. In contrast, the lower the Ea of a reaction, the greater the amount of energetic collisions present, and the faster the reaction.
Ex-for a reaction between H2 and Cl2 molecule proper orientation and activation energy are required.Without reaching the required energy the reaction cannot occur

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