Unit 3: Controlling the Rate of Reaction

Question 1

Why do industries control the rate of reaction?

Answer 1

So they aren’t too slow and economically unviable

So they aren’t too fast and risk a thermal explosion

Question 2

What do you need for successful collisions?

Answer 2

sufficient energy

correct geometry

Question 3

What affects the rate of reaction?

Answer 3

Concentration
Pressure
Particle size
Temperature

Question 4

How does concentration affect rate?

Answer 4

If you increase concentration, more particles are present in the same volume of space leading to more successful collisions

Question 5

How does particle size affect the rate?

Answer 5

If you decrease particle size, surface area increases. this means there’s a larger area for particles to collide resulting in more successful collisions

Question 6

How does pressure affect the rate?

Answer 6

If you increase pressure, volume decreases so the particles have less space to move and collide more resulting in more successful collisions

Question 7

Hows does temperature affect the rate?

Answer 7

If increase temperature there will be more particles with lower activation energy resulting in more successful collisions

Question 8

Define temperature

Answer 8

a measurement of the average kinetic energy of the particles in a substance

Question 9

Define activation energy

Answer 9

the minimum kinetic energy required by colliding particles before a reaction will occur successfully

Question 10

How do you calulate realative rate?

Answer 10

1/time

Question 11

How do you calculate the rate?

Answer 11

change in quantity/change in time