Topic 5- Kinetics

Question 1

What must happen for a reaction to take place?

Answer 1

Particle must collide.

Question 2

What is rate of reaction?

Answer 2

The change of concentration/ amount of a reactant or product per unit time.

Question 3

What is collision theory

Answer 3

For a reaction to occur particles must collide in the right direction.
Must have the minimum amount of kinetic energy.

Question 4

What is activation energy?

Answer 4

Minimum amount of energy required for a reaction to occur.

Question 5

How does temperature affect the rate of reaction?

Answer 5

Temperature
Increased
- When particles are heated they have more kinetic energy.
- Curve shifts to the right.
- Peak is lower.
- Same area under curve
- Area after activation energy is increased.
Decreased
-Curve shifts left
-Higher peak
-Area under curve is the same.
-Area after activation energy decreases.

Question 6

Why is the rate of reaction quicker at a higher temp?

Answer 6

-Particles move more at a higher temp, they collide more often therefore reactions occur faster at a higher temp.a

Question 7

How does pressure affect the rate of reaction?

Answer 7

Increasing the pressure, increases rate of reaction. As particles are closer together therefore collide more often. More frequent collisions= a higher chance of reaction.

Question 8

How does concentration affect the rate of reaction?

Question 9

What is a catalyst?

Answer 9

Increases rate of reaction by providing an alternative pathway has a lower activation energy.