9 Kinetics Flashcards
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.
