Sub Topic 1 - Rate of Reactions

Question 1

Average rate =

Answer 1

Change in * *

time

Question 2

average rate = mass/time

For mass the two numbers given are: 165.00 and 164.83. What would be the calculation carried out?

Answer 2

165.00 - 164.83/time

Question 3

The inverse relationship means

Answer 3

both variables are going in completely opposite directions.

Question 4

rate =

Answer 4

1/time

Question 5

time =

Answer 5

1/rate

Question 6

Activation energy is the

Answer 6

minimum kinetic energy required by colliding particles for a reaction to occur.

Question 7

Concentration: The closer the particles are together the

Answer 7

more chance they have of successfuly colliding and reacting

Question 8

Particle Size: The smaller the particle size, the larger the

Answer 8

surface area available for collisions to take place so a reaction is more likely

Question 9

Temperature: The higher the temperature of a substance, the higher the

Answer 9

average kinetic energy of its particles

Question 10

Energy Distribution Diagram: At any temperature the speeds (kinetic energies of molecules) are

Answer 10

spread over a wide range

Question 11

Only collisions with energy greater than

Answer 11

activation energy cna successfully produce a reaction

Question 12

Explain

Answer 12

• The higher temperature means more particles have exceeded the activation energy than at a lower temperature
• As a result more successfull collisions occur, so there are more reactions

Question 13

At a higher temperature a much larger proportion of the colliding molecules have

Answer 13

achieved the activation energy

Question 14

This means that many more molecules have the minimum energy required to collide

Answer 14

successfully and react

Question 15

A 10 degree celsius increase in temperature

Answer 15

doubles the reaction rate