Topic 8 - Kinetics 1

Question 1

What is collision theory?

Answer 1

For a reaction to occur successfully particle collisions must have energy greater than or equal to the activation energy of the reaction, and the particle orientation must be correct

Question 2

What is activation energy?

Answer 2

The minimum amount of energy required for two particles to react

Question 3

How does temperature affect rate of reaction?

Answer 3

Thermal energy is converted to kinetic energy which means the molecules move faster and further, this increased movement makes collisions more likely to occur
The increase of the particles energy means the particles are more likely to have energy greater than activation energy

Question 4

What is the affect of concentration and pressure on rate of reaction?

Answer 4

When concentration increase there is more molecules in the same volume meaning they are packed closer together. Therefore collisions will be more frequent.
Increasing the pressure (gas) packs molecules more tightly together making collisions more frequent

Question 5

Affect of surface area on rate of reaction?

Answer 5

Increasing surface area of a reactant increases the number of exposed reactant particles. This means there are more frequent and successful collisions

Question 6

Affect of catalysts on rate of reaction?

Answer 6

A catalyst is a substance that increases the rate of reaction without being used up in the reaction. It works by providing an alternative path that requires lower activation energy

Question 7

Why are catalysts used in industry?

Answer 7

1) Lower energy cost of reaction process
2) Allow lower temp and pressures to be used
3) Can give higher atom economy