1. Reversible Reactions & Dynamic Equilibria

2. Reversible or not reversible
Until now, we were careful to say that most chemical reactions were not reversible – They could not go back to the reactants once the products are formed.

3. Example
In the case of the vast majority of chemical reactions this is true, the reaction of methane and oxygen for example:
CH4(g) + O2(g)   CO2(g) + 2H2O(l)
It is almost impossible to return the carbon dioxide and water to the original methane and oxygen.

4. Reversible
Some chemical reactions, however, will go backwards and forwards depending on the conditions.
CoCl2·6H2O(s)  CoCl2(s) + 6H2O(l)
pink blue

5. How do we write them down?
This is the symbol for used for reversible reactions.
CoCl2·6H2O(s) CoCl2(s) + 6H2O(l)

6. What is equilibrium?
Reversible reactions reach a balance point, where the amount of reactants and the amount of products formed remains constant.
This is called a position of equilibrium.

7. General equation
This is the equation for a general reaction which has reached dynamic equilibrium:
How did it reach this balanced state

8. At the beginning of the reaction, the concentrations of A and B were at their maximum.
That means that the rate of the reaction was at its fastest.
A B  C D

9. As A and B react, their concentrations fall
As A and B react, their concentrations fall. That means that they are less likely to collide and react, and so the rate of the forward reaction falls as time goes on.

10. In the beginning, there isn't any C and D, so there can't be any reaction between them.
As time goes on, though, their concentrations in the mixture increase and they are more likely to collide and react.
With time, the rate of the reaction between C and D increases

11. Eventually, the rates of the two reactions will become equal.
A and B will be converting into C and D at exactly the same rate as C and D convert back into A and B again

12. At this point there won't be any further change in the amounts of A, B, C and D in the mixture.
As fast as something is being removed, it is being replaced again by the reverse reaction.
We have reached a position of dynamic equilibrium.

13. Dynamic Equilibrium.
In dynamic equilibrium the forward and backwards reactions continue at equal rates so the concentrations of reactants and products do not change.
On a molecular scale there is continuous change.
On a microscale we can’t see anything happening. We only see things on the macroscale (colours).The system needs to be closed – isolated from the outside world.