9 Kinetics
暂无描述。系统推荐的高质量记忆内容，适合每天坚持背诵学习。
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Define activation Energy:
The minimum energy required for reaction to take place between particles that collide successfully.
Why do most collisions do not lead to a reaction?
Insufficient Ea Incorrect orientation
Effect of temperature on rate of reaction:
molecules have more kinetic energy Greater proportion of molecules with Energy greater than activation energy. greater frequency of successful collisions
Effect of concentration/pressure on rate of reaction:
More particles in a given volume Particles are closer together Successful collisions are more frequent
What is a catalyst?
A substance that increases the rate of reaction by providing an alternative reaction route with a lower activation energy and is there and the start and the end without being used up.
Features of a maxwell-boltzmann distribution:
Starts from zero Highest peak is most probable energy Activation energy is dashed line further along the line. Higher Temp pushes peak down to the right. Lower Temp pushes peak up to the left. Number of molecules that reach activation energy change Catalyst pushes back activation energy line closer to axes so more particles can react.