Unit 1 - Section 5

Question 1

What is collision theory?

Answer 1

A reaction will not take place between two particles unless they collide in the right direction and with at least a certain minimum amount of kenetic energy

Question 2

What is activation energy?

Answer 2

The minimum amount of kinetic energy particles need to react

Question 3

What does a Maxwell-Boltzmann distribution show?

Answer 3

The number of molecules in a gas with different kentic energies

Question 4

What does a Maxwell-Boltzmann distribution curve look like?

Answer 4

• starts at (0,0)
• the peak of the curve represents the most likely energy of any single molecule
• the mean (average) energy is a bit to the right of the peak
• activation energy will be shown, any molecules after this point would be able to react

Question 5

What is the effect of temperature on reaction rates?

Answer 5

If you increase the temperature the molecules average will be moving faster so will move to the right, also the curve will be less steep on ever side and will have more molecules over the activation energy point

Question 6

What is the effect of concentration on reaction rates?

Answer 6

The curve is steeper and higher. It is not steeper on the right side and therefore has an increase in the amount of molecules over the activation energy but it drops to the same amount as before

Question 7

What is a catalyst?

Answer 7

The catalyst increases the rate of reaction by producing an alternative reaction pathway with a lower activation energy

Question 8

How are reaction rates calculated?

Answer 8

Amount of reactant used or product formed
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Time