1. Chemical Equilibrium

2. Intro:
Many chemical reactions go to completion (where all reactants are consumed to form product)
This unit deals with reactions that do not completely convert all reactants to products.

3. Chemical Equilibrium
A state where the rate of the forward chemical reaction is equal to the rate of the reverse chemical reaction
Double arrows show that a system is at equilibrium

5. Characteristics of a system at equilibrium
Reversible reaction must be possible
There is a dynamic state of balance between both the forward and backward reaction
There is no change in concentration of reactants or products once chemical equilibrium is reached
There is no bulk change in properties of the system (ex: no colour or pressure change)

6. Characteristics cont.
It is a closed system (no heat or matter in or out)
The temperature of the system remains constant
It can be reached from either direction
Any change to the system at equilibrium can be reversed if restored back to original equilibrium conditions.

7. Examples at Equilibrium
Water evaporating and condensing in a jar with lid.
Any solution at the saturation point.
A bottle of unopened pop, carbon dioxide is in equilibrium in solution and air above pop.
Walking the wrong way on an escalator.

8. Equilibrium System Simulation
With a partner, take two graduated cylinders and fill them with a random amount of water (not full).
Record the volume of water in each cylinder.
Take straws and place one into each of the cylinders, wet your finger and place it on the top of the straw.
Transfer the water trapped in the straw to the other cylinder (do not spill).
Record new volume in each cylinder.
Repeat until the volumes are unchanged for three trials.
Plot a graph of volume vs trials

9. Analysis
How were you able to tell when your system established equilibrium?
Would the system be described as an open or closed system?
How does this simulation model a dynamic equilibrium system?

10. Homework
Read Section 7.1
Page 428 #1,2

12. Changing the temperature affects the rates of forward and reverse reactions differently because they have different activation energies
Kc = expressed in terms of molar concentration (mol/L)

16. Calculating Kc N2 + 3Cl2 <--> 2NCl3
Temp remains constant in 5 L flask.
Equilbrium was reached and the following was found: mol N2 , mol Cl2 and 0.95 mol of NCl3. Calculate the Kc for this reaction.
Find molar concentration of everything (mol/L)
Use equilibrium expression based on chemical equation

17. Answer
[N2] = mol / 5 L = M
[Cl2] = mol / 5 L = M
[NCl3] = 0.95 mol / 5 L = 0.19 M
Kc = [NCl3]2 = [0.19]2
[N2][Cl2]3 [0.0014][ ]3
= 3.0 x 10 11

18. CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
1. Write an expression for Keq 2. Calculate K at a given temperature if [CH4] = M, [O2] = M, [CO2] = M, and [H2O] = M at equilibrium. (include units)

19. K eq = 0.306
Time to practice…

20. Practice:
Read section 7.2
Pg 431 #1-3
Pg 436 #2,3

21. The value of K
The value or magnitude of K tells us the extent to which reactants have been converted into products.
Remember in the ratio for K, the concentration of products divided by the concentration of reactants.

22. A small value for K means that very little of the reactants were converted into products before equilibrium was reached.
This is stated as “reactants are favoured”.
A large value of K means that most of the reactants were converted into products before equilibrium was reached.
This is stated as “products are favoured”.

23. The Magnitude of Equilibrium Constants
If K >1, then products dominate at equilibrium and equilibrium lies to the right.
If K <1, then reactants dominate at equilibrium and the equilibrium lies to the left.

24. If K = 1 neither reactants nor products are favoured. The value of
K does not indicate how long it takes for equilibrium to be reached. The value of K varies with temperature and that’s why its usually mentioned with K

25. 2NO2 (g) <--> N2O4 (g)
Four experiments were performed.
The initial concentrations of the two chemicals were
different in each experiment and the concentration of each gas was measured once the system reached equilibrium.
At Equ
ilibrium
Exp #
[NO2]
[N2O4] 1
0.104
1.19 2
0.048
0.254 3
0.136
2.04 4
0.202
4.48

26. Calculate
Using the data on the previous page, calculate the K for each experiment.
What did you find?

27. Homework