Collision theory and activation energy

Question 1

collision theory

Answer 1

chemical reactions only occur when reacting particles collide with each other and with sufficient energy

Question 2

activation energy

Answer 2

the minimum amount of energy that particles must have to react

Question 3

factors affecting rates of collisions

Answer 3

temperature
concentration of reactants
pressure of reacting gases
surface area of solid reactant

Question 4

Why increasing temperature has an effect

Answer 4

particles have more energy
particles move faster
more collisions per second
collide with more energy

Question 5

why increasing concentration/pressure has an effect

Answer 5

more particles in the same space so more frequent collisions

Question 6

why increasing surface area has an effect

Answer 6

more particles exposed to other reactants so more frequent collisions

Question 7

catalyst definition

Answer 7

a substance that speeds up a chemical reaction without being used up> Adding a catalyst to a reaction increases the rate of reaction

Question 8

why do catalysts work?

Answer 8

They provide a different pathway for the reaction that has a lower activation energy.
they reduce the amount of energy needed for particles to collide successfully.