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The rate of reaction increases as the twmperature increases. Which of the following statement provides the best explanation for this?

Sagot :

Answer:

According to Collision Theory

Reactions can only happen when the reactant  particles collide, but most collisions are NOT successful in forming  product molecules despite the high rate of collisions. It can only be successful with effective collision.  Effective collision means reactants  should have sufficient energy, and their molecules should be in proper  orientation for a successful collision to happen.  The minimum kinetic energy required for reaction is known as the activation energy.

So when there is an increases in temperature, the kinetic energy in the reactant increases which resulted to sufficient energy in the reactant because it only needs less activation energy since the reactant already increases its kinetic energy due to  increase in temperature.

Explanation:

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