Understanding Collision Theory and Activation Energy for Chemical Reactions

The video explains collision theory, which states that particles must collide with sufficient energy for a reaction to occur. This energy is known as activation energy. The rate of reaction depends on the number of collisions with energy exceeding the activation energy. To increase reaction rates, one can increase the number of particles or the energy of the particles, leading to more frequent and energetic collisions.

How does increasing the number of particles affect the likelihood of collisions?

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Describe how increasing the energy of particles influences chemical reactions.

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