Collision Theory and Rates of Reaction"

Question 1

In order for particles to react what must they do?

Answer 1

= collide with eachother- cannot react otherwise
= chemical bonds must be broken, particles must collide with enough energy to do so
= particles must collide with the correct orientation

Question 2

What is the activation energy?

Answer 2

= minimum amount of energy required for a sucessful chemical reaction (collisions) to occur

Question 3

What happens if collisions do not have enough energy?

Answer 3

= the particles cannot react
= bounce off eachother

Question 4

What is the rate of reaction porportional to?

Answer 4

= number of effective collisions

Question 5

What is one way we can increase the rate of reaction ?

Answer 5

= increasing the concentration
= increases chance of collisions occuring- closer togethr exposure
= increased frequency of collisions
= reaction occurs

Question 6

What is the second way of increasing the rate of reaction?

Answer 6

= increasing pressure (gas)- particles closer together, increasing frequence of collisions