KINETICS

Question 1

define activation energy

Answer 1

the minimum amount of energy required for reaction to take place.

Question 2

What is the collision theory?

Answer 2

The collision theory states reactions can only occur when collisions take place between particles that have sufficient energy.The energy is required to break the relevant bonds of the reactant molecules.

Question 3

How does increasing the temperature effect rate of reaction?

Answer 3

*rate of reaction increases
By increasing the temperature more particles have greater than or equal to (≥)activation energy therefore we have more successful frequent collisions.

Question 4

Explain the effect of lowering the temperature would have on the rate of reaction?

Answer 4

• rate of reaction decreases
• fewer particles would have greater than or equal to(≥)activation energy
• therefore less frequent and successful collisions

Question 5

Explain the effect of decreasing the concentration(or pressure) has on the rate of reaction:

Answer 5

• rate of reaction decreases
• particles are spread further apart
• Fewer collisions between particles so fewer successful collisions

Question 6

Explain the effect of increasing concentration (or pressure) has on effect on the rate of reaction:

Answer 6

• increases rate of reaction
• increasing pressure or concentration increases the number of molecules in a given volume,so molecules are closer together
• More successful and frequent collisions

Question 7

Explain the effect of Increasing Surface Area:

Answer 7

Increasing the surface area increases the area which a reaction can occur and will cause successful collisions to occur more frequently between the reactant particles and this increases the rate of the reaction.

Question 8

How does a catalyst increase the rate of reaction?

Answer 8

a catalyst increases rate of reaction without getting used up.Catalyst provide an alternative pathway that has a lower activation energy.