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Chapter 16: Problem 114

What does the activation energy for a reaction represent? How is the activation energy related to whether a collision between molecules is successful?

Short Answer

Expert verified
The activation energy represents the minimum amount of energy required for a chemical reaction to occur. It determines the likelihood of a successful collision between molecules, as a reaction can only occur if the molecules' kinetic energy is equal to or greater than the activation energy. A higher activation energy reduces the likelihood of a successful collision, while a lower activation energy increases it. Catalysts can lower the activation energy, and increasing the temperature can increase the number of successful collisions by raising the kinetic energy of molecules.

Step by step solution

01

Understanding Activation Energy

The activation energy refers to the minimum quantity of energy that the reacting species must possess in order to undergo a specified reaction. In other words, it's the energy required to start a chemical reaction.
02

Relation of Activation Energy to a Successful Reaction

A successful collision between molecules which leads to a reaction only occurs if the kinetic energy of the molecules is equal to or greater than the activation energy. The larger the activation energy, the less likely a collision will result in a reaction because fewer molecules will have the necessary energy. Conversely, a lower activation energy means that more molecules will have the required kinetic energy, increasing the chances of a successful reaction.
03

Role of Catalysts in Activation Energy

Catalysts are substances that lower the activation energy of a reaction. They work by providing a different path with a lower activation energy for the reaction. This allows more collisions to result in a reaction, thereby speeding up the reaction rate.
04

Temperature Impact on Activation Energy

Increasing the temperature, typically, increases the kinetic energy of the molecules, which increases the number of molecules that have enough energy to exceed the activation energy. Therefore, increasing the temperature generally increases the rate of reaction due to a greater probability of successful collisions. Through this explanation, you should now have a solid understanding of what activation energy represents and how it relates to a successful collision between molecules during a reaction.

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