Rates of reaction

Question 1

What is activation energy?

Answer 1

minimum energy required to start a reaction by breaking bonds

Question 2

what is collision theory?

Answer 2

Two reacting particles must collide for a reaction to occur, and must be in the correct orientation and have sufficient energy to overcome the activation energy of the reaction

Question 3

what are the benefits of using catalysts?

Answer 3

• can make reactions take place rapidly even at low temperatures = reduces amount of energy needed = reduces need to burn fossil fuels to supply energy = saves money + reduces carbon dioxide emissions

Question 4

what are the risks of using catalysts?

Answer 4

some catalysts are toxic

Question 5

how do you measure the rate of a reaction?

Answer 5

look at how fast reactants are being used up OR how fast products are being formed

Question 6

what does the presence of a catalyst do?

Answer 6

lowers activation energy by providing an alternative pathway = greater proportion of particles will collide with enough energy to overcome activation energy

Question 7

what happens to catalysts in a reaction?

Answer 7

catalysts ARE NOT used up + ARE NOT permanently changed = can be reused

Question 8

what are the factors that impact the rate of reaction?

Answer 8

concentration
pressure
surface area
temperature
catalyst

Question 9

what is a transition state?

Answer 9

some chemical bonds are being broken and some chemical bonds are being formed