Kinetics

Question 1

what must particles do in order to react?

Answer 1

particles must collide with sufficient energy (activation energy) and the correct orientation.

Question 2

do must collisions result in a reaction?

Answer 2

NO

Question 3

define activation energy?

Answer 3

the minimum amount of energy needed for particles to collide for a reaction.

Question 4

what is the effect of increasing the temperature on the rate of reaction? Why?

Answer 4

increasing temp —> increases the rate of reaction
higher proportion of particles have higher energy than the Ea which causes many more successful collisions per second and increases the rate of reaction.

Question 5

what is the effect of increasing pressure/concentration on the rate of reaction?Why?

Answer 5

increasing concentration/pressure —> increases rate of reaction
there are more particles in a given volume which leads to more frequent collisions and increased rate of reaction.

Question 6

what is a catalyst?

Answer 6

A substance which increases the rate of reaction but is not used up in the reaction.

Question 7

How do catalysts work and how do they increase the rate of reaction?

Answer 7

Catalysts lower the activation energy so more particles have energy higher than the activation energy, so more frequent successful collisions, so increased reaction rate.
Provides and alternative pathway ( one with a lower activation energy)

Question 8

Draw a labelled maxwell - boltzman curve.

Answer 8

diagram