Kinetics (P2+P3)
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Define activation energy
the minimum energy needed for a reaction to occur.
Why do most collisions not cause a reaction?
a small number of particles have E>Ea (collision energy greater than activation energy)
What is the rate of reaction?
the rate of change in concentration per unit of time
How does a temp increase cause an increase in rate?
more particles have E>Ea more successful collisions
How does a concentration and pressure increase cause an increase in rate?
increase in number of particles per unit volume more successful collisions
How does the addition of a catalyst increase the rate of reaction?
lowers activation energy so more particles have collision energy greater than the activation energy so more successful collisions
What is a catalyst?
substance that increases the rate of reaction but is not used up
How does a catalyst work?
lowers activation energy by providing an alternative reaction route.