1. CHEMICAL EQUILIBRIUM
My faith helps me overcome such negative emotions and find my equilibrium.
- Dalai Lama

2. Reactions are Reversible
A + B  C + D (forward)
Initially there is only A and B so only the forward reaction is possible
As C and D build up, the reverse reaction speeds up while the forward reaction slows down.
C + D  A + B (reverse)
Eventually the rates are equal

3. Forward Reaction
Reaction Rate
Equilibrium
Reverse reaction
Time

4. What is equal at Equilibrium?
The Forward and Reverse Reaction Rates are equal.
Forward and Reverse Reactions are still occurring.
Concentrations are NOT necessarily equal.
The concentrations of reactants and products do not change at equilibrium.

5. Ratio of Reactant to Products at EQ
At equilibrium, there is a set ratio of product concentrations to reactant concentrations
This ratio is given by K, the equilibrium constant
K is unique for a particular temperature.
Since an increase in temperature usually favors either the forward or reverse reaction (whichever is endothermic), K value changes as the temperature changes.

6. Law of Mass Action For any reaction jA + kB lC + mD
Keq = [C]l[D]m PRODUCTSpower [A]j[B]k REACTANTSpower
Keq is called the equilibrium constant.
Keq is commonly written as Kc since concentrations are used to determine the Keq.

7. Mass Action Expression
2 HCl (g) H2 (g) + Cl2 (g)
Keq or Kc =
N2 (g) + 3 H2 (g) 2 NH3 (g)

8. K Values K > 1: products are "favored"
K = 1: neither reactants nor products favored
K < 1: reactants are "favored“
T This reaction has a large K value.

9. Keq is constant at a certain T
Regardless of what we begin with, the ratio of products to reactants is constant at equilibrium

10. K of the reverse reaction
Write the reaction in reverse.
lC + mD jA + kB
Then the new equilibrium constant is
Krev = [A]j[B]k = 1/Kfor [C]l[D]m
If the Keq is 5.0 x 103, what is the Keq of the reverse reaction?

11. The units for K There is no set or common unit for K.
The units are dependent on the reaction.
There may be no units, M, M2, 1/M, etc.
Since units may vary, the standard method is to not include any units.

12. Solving Problems AT Equilibrium
Using the Mass Action Expression

13. Calculate Kc
N2 + 3H2 2 NH3 Initial At Equilibrium [N2] = M [N2] = 0.921M [H2] = M [H2] = 0.763M [NH3] = 0.0 M [NH3] = 0.157M

14. Calculate Kc N2 + 3H2 2 NH3 Initial At Equilibrium
[N2] = 0.0 M [N2] = M
[H2] = 0.0 M [H2] = M
[NH3] = M [NH3] = 0.157M
K is the same regardless of starting concentrations as long as temperature remains constant.

15. A Slightly Tougher K Problem
3.00 moles of pure SO3(g) are introduced into an 8.00 dm3 container at 1105 K. At equilibrium, 0.58 mol of O2(g) has been formed.
2SO3(g)         2SO2(g) + O2(g)
Calculate Kc
What other information must we first gather? 15

16. ICE Table 2SO3(g) 2SO2(g) + O2(g) SO3(g) SO2(g) O2(g) Initial moles
SO3(g)
SO2(g)
O2(g)
Initial moles
3.00
Change moles
-2y
+2y +y
Equilibrium moles
( )
1.16
0.58
Equilibrium concentrations 
1.84/8.00 
1.16/8.00 
0.58/8.00 
2SO3(g)        2SO2(g) + O2(g) 16

17. CdI42- (aq) Cd2+ (aq) + 4 I- (aq)
Practice Problem 1
An aqueous solution is prepared that is initially M CdI42- After equilibrium is established the solution is found to be M in Cd2+.
CdI42- (aq)  Cd2+ (aq) + 4 I- (aq)    
Derive the expression for the equilibrium expression and calculate the value of the constant?

18. MgF2 (s) Mg2+ (aq) + 2 F- (aq)
Practice Problem 2
In a saturated solution of MgF2 at 18°C, the concentration of the Mg2+ is 1.21 x 10-3 molar. The equilibrium is represented by the equation below.
MgF2 (s) Mg2+ (aq) F- (aq)
Derive the expression for the equilibrium expression and calculate the value of the constant at 18ºC.

19. Practice Problem 3 CH3COOH CH3COO- + H+
In a solution of acetic acid, the equilibrium concentrations are found to be [CH3COOH] = 1.000, [CH3COO-] = , and [H+] =
Calculate the Ka of acetic acid.
What is the pH of this solution? (pH = -log[H+]) 19

20. CO2 (g) + H2(g) H2O (g) + CO (g)
Practice Problem 4
When H2 (g) is mixed with CO2 (g) at 2000 K, equilibrium is achieved according to the equation.
CO2 (g) + H2(g)     H2O (g) + CO (g)
Determine the value of the equilibrium expression if, at equilibrium, [H2] = 0.20 M, [CO2] = 0.30 M, [H2O] = 0.55 M, and [CO] = 0.55 M.
If the temperature is lowered, the [CO] becomes 0.40 M. Calculate the value of Kc at this lower temperature.
What is the Kp of this reaction at 2000K?

21. Converting from Kc to Kp
Kp = Kc(RT)Δn
Kp = Equilibrium constant based on pressure
Kc = Equilibrium constant based on molar conc.
R = Gas constant, use L atm mol-1 K-1
T = Temperature, use Kelvin temp
Δn = moles product gas – moles reactant gas

22. Tough Problem
4.00 moles of HI are placed in an evacuated 5.00 L flask and then heated a 800K.  The system is allowed to reach equilibrium. 
2 HI(g)   H2(g) + I2(g)   
What will be the equilibrium concentration of each species if Kc = at 800K?

23. ICE, ICE, baby! HI H2 I2 .80 0 0 - 2x + x + x .80 - 2x + x + x
2 HI(g)   H2(g) + I2(g) 
HI H2 I2
Initial
Change EQ
- 2x + x + x
x x x
(x) (x) =
x = via the quadratic equation
(.8 - x)2