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Describe the differences between the rate of reaction at different concentrations and collision theory.

The rate of reaction at different concentrations is explained by collision theory.

Collision theory explains how different factors affect the rate of chemical reactions. One of these factors is the concentration of reactants. According to collision theory, the rate of reaction increases with an increase in the concentration of reactants. This is because as the concentration of reactants increases, the number of collisions between them also increases. This leads to a higher probability of successful collisions, resulting in a faster rate of reaction.

The theory also explains that not all collisions between reactant molecules result in a successful reaction. For a reaction to occur, the colliding molecules must have enough energy to break their existing bonds and form new ones. This is known as the activation energy. The higher the concentration of reactants, the more collisions occur, increasing the chances of successful collisions with enough energy to overcome the activation energy barrier.

In summary, the rate of reaction at different concentrations is explained by collision theory. An increase in concentration leads to an increase in the number of collisions between reactants, increasing the probability of successful collisions with enough energy to overcome the activation energy barrier.

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