Question

What happens to the rate of the reaction when the concentration is increased? Explain the effect of concentration on reaction rate in terms of collision theory. Your answer should include at least four complete sentences.

Answer 1

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Increasing the concentration would increase the rate of reaction. This is because there would be more particles.Therefore, there would be an increase in the rate of successful collisions per second. More successful collisions would mean that the reaction occurs much quicker.

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Answer 2

Answer:

When the concentration is increased, the rate of the reaction will increase.

Explanation:

Collision theory is a model to explain the mechanisms of chemical reactions. In order for a chemical reaction to occur, the breaking of bonds between the atoms of the reagent molecules and the formation of new bonds are generated in order to originate the molecules of the products. Then the molecules of the reagents must collide, so, the greater the number of shocks, the faster the reaction rate. This is summarized in: "The speed of a reaction is proportional to the number of collisions produced per unit of time between the reagent molecules."

But for the shocks to be effective they must be produced with enough energy to break and form chemical bonds. This energy is called activation energy. Also in the crash there must be a proper orientation or direction for the reaction to take place.

Finally, the number of shocks between the reactant species is proportional to the concentration of the reagents. This means that by increasing the concentration of the reagents the number of collisions will be greater. This increases the speed of the reaction.