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

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

Answer 4

Find the answer to this on PMT slide 9 kinetics

Question 5

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

Answer 5

1. Increasing temperature => increased rate of reaction
2. 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 rater 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

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