Kinetics (P2+P3)

Question 1

Define activation energy

Answer 1

the minimum energy needed for a reaction to occur.

Question 2

Why do most collisions not cause a reaction?

Answer 2

a small number of particles have E>Ea (collision energy greater than activation energy)

Question 3

What is the rate of reaction?

Answer 3

the rate of change in concentration per unit of time

Question 4

How does a temp increase cause an increase in rate?

Answer 4

more particles have E>Ea
more successful collisions

Question 5

How does a concentration and pressure increase cause an increase in rate?

Answer 5

increase in number of particles per unit volume
more successful collisions

Question 6

How does the addition of a catalyst increase the rate of reaction?

Answer 6

lowers activation energy
so more particles have collision energy greater than the activation energy
so more successful collisions

Question 7

What is a catalyst?

Answer 7

substance that increases the rate of reaction but is not used up

Question 8

How does a catalyst work?

Answer 8

lowers activation energy by providing an alternative reaction route.