1. Chemical Kinetics and Equilibrium

2. Reaction Rates
How fast or slow the reaction occurs

3. Collision Theory
2 conditions must be satisfied for a chemical reaction to occur
Particles of reactants must collide with one another; and
Colliding particles must have sufficient energy

4. Activation Energy F> Ea Ea
Minimum amount of energy needed for a reaction to occur
F> Ea Ea

5. F < Ea Ea

6. Energy Diagram for Exothermic reaction
increasing Average energy
energy of reactants
Energy difference bet Average energy
reactants and products of products

7. Energy Diagram for Endothermic reaction
increasing
energy
energy of the products
energy of
reactants energy difference

8. Factors Affecting Rate of reaction
Surface Area
Concentration of reactants
Temperature
Presence of Catalyst

9. Surface area of reactants
Consider the block of wood or wood shavings
The smaller the particle size of wood the greater the surface area exposed to oxygen thus the rate of reaction increases.

10. Concentration of Reactants
An increase in concentration of the reactants causes an increase in the rate of chemical reaction

11. Temperature Higher temperature increases reaction rates
Ex: ripe fruits are placed in the refrigerator to slow down the ripening process.

12. Presence of Catalyst Catalyst
Substance that speeds up chemical reaction without itself undergoing a chemical change
Inhibitor
--->substances that slow down reaction

13. Activation energy of uncatalized reaction
catalyzed activation energy
Uncatalyzed
activation energy
Note: Catalysts increases
reaction rates by
providing alternative
reaction pathways
with lower activation
energies

14. Lower activation energy
Means that a lower amount of energy is needed to surpass the energy barrier.

15. Chemical Equibrium
It is always assumed that chemical reaction go to completion
However, only few chemical reactions proceed to completion
Reversible reaction
N2O4(g) NO

16. Reversible Reaction N2O4(g) 2NO2
A chemical reaction in which the products can regenerate the original reactants
N2O4(g) NO2
colorless brown
N2O4(g) > 2NO2(g) ( forward Reaction)
2NO2 (g) > N2O4(g) (backward Reaction)

17. Chemical Equilibrium
The rate of forward reaction and backward reactions are equal
Is dynamic
 The reactants constantly forms the products while the products constantly forms the reactants
Note:
In equilibrium, concentration of reactants and products do not change

18. Ex: dynamic Equilibrium
Carbonated Drinks
CO2 + H > H2CO3
carbonic acid
When the bottle is opened the pressure is released, carbon dioxide evolved from the decomposition of carbonic acid
H2CO > CO2 + H2O
CO2 + H H2CO3

19. Equilibrium Constants(K)
Can be obtained in any equilibrium reaction
Equal to the Ratio of the equilibrium concentration of the products to the equilibrium concentration of the reactants
aA + bB ----->cC + dD
Where:
a,b,c & d -- are the coefficients
A,B,C & D– are the chemical species

20. Equilibrium Constant(K)
aA + bB ----->cC + dD
K = [C]c [D]d = [ products ]
[A]a [B]b [reactants]
--> Experimentally at equilibrium, Concentration of the products raised to a certain power divided the concentration of the reactants also raised to a certain power is constant at( fixed temperature)
Is also called equilibrium expression

21. Note: K = [ products] [reactants]
is the concentration of products over that of the reactants
If the K value is small, it means that the equilibrium concentration of the products is small while the reactants are large. This indicates that at equilibrium, the system consist mostly of reactants
If the K value is great , it means that the equilibrium system consist mostly of the products

22. Writing equilibrium expression
If a pure liquid or solid is involved in a reaction, its concentration is omitted in the equilibrium expression because it has constant concentration in mol/L at constant Temperature

23. Ex: Write the equilibrium expression for the reaction below
H2(g) + F2(g) HF(g)
K = [ HF]2
[H2] [F2]

24. Ex:2 Write the equilibrium expression for the reaction below
N2(g) + 3H2(g) NH3(g)
K = [NH3]2
[N2][H2]3

25. Ex:3 Write the equilibrium expression for the reaction below
CaCO3(s) CaO(s) +CO2(g)
K = [ CO2]

26. Ex:4 Write the equilibrium expression for the reaction below
2Hg(l) + O2(g) HgO(s)
K = since solid and liquid is omitted
[O2]

27. Exercises Write the expression of the following Reactions
2H2S(g) + 3O2(g) 2H2O(g) + 2SO2(g)
CO2(g) + H2(g) ---> CO(g) + H2O(l)
FeO(s) + H2(g) --->

28. Le Chatelier’s Principle
States that if a change in conditions is imposed on a system at equilibrium, the equilibrium position will shift in the direction that tends to reduce the effects of that change
-->The effect of change in concentration
 The effect of change in Volume
The effect of change in temperature

29. Effects of Change in Concentration on reaction Equilibrium
Consider the equation below
N2 + 3H NH3(g)
This equation shows equilibrium because of the two arrows of the same length that is rate of forward reaction is equal to the rate of backward reaction.
What will happen if you increase the concentration of N2?
increasing the concentration of the reactants means more collision between them that increases the rate of forward reaction as shown below
N2 + 3H NH3(g)
Notice that the arrow pointing to the right has a greater length which indicates forward reaction increases meaning more production of NH3

30. What happens if you increase the concentration of NH3 in the previous example?
N2 + 3H NH3(g)
Increasing the concentration of NH3 will shift the reaction to the left.
Note:
If a reactant or product is added to the system, the system shifts away from the added component
If a reactant or product is removed, the system shifts toward the removed component

31. Exercise Suppose the reaction system 2SO2(g) + O2(g) 2SO3 (g)
Has reached equilibrium. Predict the effect of each of the following changes on the position of the equilibrium
a) SO2(g) is added to the system
Ans. Shift to the right( forward)
b) The SO3(g) present is liquefied and removed from the system
Ans. Shift to the right(forward)
b)Some of the O2 gas is removed from the system
Ans. Shift to the left ( backward)

32. The effect of Change in Volume and pressure
Recall :
Boyle’s law : Pressure is inversely proportional to Volume of gases
The smaller the volume, the higher the pressure between molecules
Avogadro’s Law : V is directly proportional to the # of moles at constant T
Consider the equation below: suppose the gases below are mixed in a vessel
at equilibrium
2 NOCl(g) NO(g) + Cl2(g)
What will happen to the equilibrium position if we reduce the volume?
Reducing volume means increasing the pressure between the molecules of the gases, the system moves in the direction that lowers its pressure. In the equation above, the direction will shift to the left because the products has more molecules (3 molecules) than the reactant (2molecules).
In other words, the equilibrium position will shift toward the side of the reaction that involves the smaller number of gaseous molecules in the balanced equation

33. What happens when volume is increased in the previous example?
2 NOCl(g) NO(g) + Cl2(g)
When the volume is increased, it lowers the pressure of the system, thus the direction will shift to the right to increase the total number of gaseous molecules present

34. Predict the shift in equilibrium of the reaction below when volume is reduced
a) P4(s) + 6Cl2(g) PCl3(l)
6 gaseous molecules gaseous molecules
The direction will shift toward the right since it has 0 gaseous molecules
b) PCl3(g) + Cl2(g) PCl5(g)
2 gaseous molecules gaseous molecule
The direction will shift to the right since it has lesser number of gaseous molecules
c) PCl3(g) + 3NH3(g) P(NH2)3(g) + 3HCl(g)
4 molecules molecules
Since the # of gaseous molecules in both sides are equal, a change in volume will have no effect on the equilibrium position

35. Practice:
For each of the following reaction predict the direction in which the equilibrium will shift when volume in the container is increased
a) 4NH3(g) + 5O2(g) NO(g) + 6H2O(g)
b) FeO(s) + H2(g) Fe(s) + H2O(g)

36. The effect of change in Temperature
The change in concentration and volume in the system alter the equilibrium position but not the equilibrium constant (K)
The effect of temperature on equilibrium is different because the value of equilibrium constant (K) is change
If the reaction is exothermic that means it releases heat the direction will shift to the left since heat is is one of the products
A) C(s) + O2(g) < > CO2(g) + heat
direction will shift away from heat( to the left)
If the reaction is endothermic, energy is one of the reactants so the direction will shift to the right

37. Exercise:
Predict the shift would each of the changes below have on the reaction
O2(g) + 2CO(g) CO2(g) + heat
a)Increasing [CO]
b)Increasing [CO2]
c) Increasing Temperature
d) Decreasing volume