Kinetics - Physical 1

Question 1

What must particles do in
order to react?

Answer 1

Collide with sufficient energy (activation energy)
and the correct orientation

Question 2

Do most collisions result in
a reaction?

Answer 2

no!!

Question 3

Define Activation Energy.

Answer 3

The minimum energy that particles must collide
with for a reaction to occur

Question 4

Draw a labelled Maxwell-Boltzman
Curve. Label average energy, activation
energy and most probable energy.
Draw in a different colour the effect of
increasing temperature

Answer 4

CHECK THE INTERNET ETC!!!!!!

Question 5

What is the effect of
increasing temperature on
rate of reaction? why?

Answer 5

Increasing temperature → increased rate of
reaction
Much higher proportion of particles have energy
greater than the activation energy → many more
successful collisions per second →increased rate

Question 6

What is the effect of
increasing
concentration/pressure on
rate of reaction? why?

Answer 6

Increased concentration/pressure → increased rate of
reaction
There are more particles in a given volume → more frequent
successful collisions → increased rate

Question 7

What is a catalyst?

Answer 7

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

Question 8

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

Answer 8

Provide an alternative reaction pathway (one with a lower
activation energy)
Lowers activation energy, so more particles have energy >
activation energy, so more frequent successful collisions, so
increased reaction rate