Kinetics

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

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

Answer 4

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 5

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

Answer 5

Increased concentration/pressure → increased rate of reaction

There are more particles in a given volume → more frequent successful collisions → increased rate

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

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.