R2.1 - how fast? the rate of chemical change

Question 1

What is a rate?

Question 2

What is a rate of reaction?

Question 3

What is a tangent?

Question 4

What are the 6 methods of measuring rates of reactions?

Question 5

How do you calculate rate of reactions?

Question 6

What is the kinetic molecular theory of matter?

Question 7

What is absolute temperature?

Question 8

What is the relationship with temperature and kinetic energy?

Question 9

What happens to kinetic energy and temperature as you move from solid to gas?

Question 10

What is the Maxwell-Boltzmann energy distribution curve?

Answer 10

shows the number of particles having a specific value of kinetic energy against the values of kinetic energy

Question 11

What does the Maxwell-Boltzmann curve tell us about distribution?

Answer 11

• large number of molecules with less energy
• small number of molecules with more energy

Question 12

What is required for a reaction to occur?

Answer 12

• enough energy
  
  • correct orientation

Question 13

What is activation energy?

Answer 13

minimum value of kinetic energy which particles must have so that they can react
- energy is required so that the transition state between reactants and products can occur

Question 14

What 5 factors affect the rate of reaction?

Answer 14

• temperature
• surface area
• pressure
• volume
• catalysts

Question 15

How can temperature affect the rate of reaction?

Answer 15

as temperature increases, the number of molecules that have significant activation energy increases (area under the line to the right increases) and so does kinetic energy
- collision frequency also increases as the particles will be moving faster so there will be more successful collisions

Question 16

How can temperature affect the Maxwell-Boltzmann curve?

Question 17

How can concentration affect the rate of reaction?

Question 18

How can concentration change be seen in a graph?

Question 19

How can pressure affect the rate of reaction?

Question 20

How can pressure change be seen on a graph?

Answer 20

• same amount of product made
• less steep for a lower pressure

Question 21

How can surface area affect the rate of reaction?

Answer 21

smaller solids –> surface area increases
- this means that there is a larger surface area for particles to collide on, increasing the chance of successful collisions and the rate of reaction

Question 22

How can surface area change be seen in a graph?

Question 23

How can catalysts affect the rate of reaction?

Question 24

How can catalysts be seen on the Maxwell-Boltzmann curve?

Question 25

What are systematic errors?

Question 26

What are random errors?