1. Topic 8: Kinetics and Equilibrium

2. Kinetics
Kinetics: the branch of chemistry that is concerned with the rates of chemical reactions.
In order for a reaction to occur, reactant particles must collide-this is called collision theory.
Collisions between particles must be effective.

3. The following factors affect the rate of reaction by changing the number of effective collisions that place between particles.
Nature of the reactants: - Substances with covalent bonds react SLOWER than ionic substances due to the greater number of bonds.
Concentration- Most chemical reactions will occur at a rapid rate if the concentration of one or more reactants is increased.
Surface Area- When more surface area of a substance is exposed, there are more chances for reactant particles to collide thus contributing to a faster rate of reaction

4. The Presence of a Catalyst- Catalyst are substances that increase the rate of reaction (Forward and Reverse) by providing a different and easier pathway for a reaction. Unchanged when the reaction is complete.
Temperature- At a higher temperature: more collisions, and more energy, making it more likely that the collisions will be effective.
Pressure- Has no effect on the rate of reaction of liquids or solids.
-It does have an effect on gases. Increase in pressure increases the rate of reaction of gases.

5. Potential Energy Diagram
A- Potential energy of the reactants.
B- Potential energy of the activated complex.
C- Potential energy of the products.
D- Difference between the potential energies of the products and the activated complex.
E- Potential energy of the activated complex when a catalyst is present.
F- Difference between the potential energies of the products and the activated complex.
G- Difference in potential energy between the reactants and the activated complex.
Activation energy: the amount of energy needed to form the activated complex from the reactants.

8. Potential Energy Diagram
As a reaction proceeds toward the product side, two outcomes are possible
As the activated complex changes to become the product it will lose energy.
If the product has more potential energy than the reactants, the reaction will be endothermic - meaning there is a net gain of energy.
If the product has less potential energy than the reactants, the reaction will be exothermic - meaning there is a release of energy.

9. Equilibrium
When both the forward and reverse reactions occur at the same rate it is called equilibrium.
An equation representing equilibrium uses a double arrow instead of a single arrow to show that reactions are proceeding in both directions.

10. Equilibrium Equilibrium:
A state of balance between the rates of two opposite processes that are taking place at the same rate.
Can only occur in a system in which neither reactants nor products can leave the system.
It is a dynamic process- implies motion in which the interactions of reactant particles are balanced by the interactions of product particles.
An important concept because many chemical reactions and physical processes are reversible- they are able to proceed in both directions.
It must be emphasized that the quantities of reactants and products are not necessarily equal at equilibrium, it is the rates of the two reactions, forward and reverse, that are equal.

11. Equilibrium
Physical Equilibrium: can occur during physical processes such as change of state (phase) or dissolving
Phase Equilibrium: can exist between the solid and liquid phases of a substance. This condition is defined as the melting point of the solid phase or the freezing point of the liquid phase. A similar relationship can exist in a closed container for liquid-gas equilibrium, where the rate of evaporation is equal to the rate of condensation.
Solution Equilibrium: Solids in equilibrium exist in equilibrium in a saturated solution. When the rate of dissolving and recrystallizing are equal, equilibrium exists, and the solution is saturated. Equilibrium may also be reached in a closed system between a gas dissolved in a liquid and the undissolved gas.

12. Equilibrium
When reactants are first mixed and no products are present, only the forward reaction can occur. As time progresses, the concentrations of the reactants decrease, causing the forward reaction to slow, while the concentrations of the products increase which causes the rate of the reverse reaction to increase.
This slowing of the forward reaction and speeding up of the reverse reaction continues until the rates of the two reaction become the same, meaning chemical equilibrium exists.

13. Le Châtelier’s Principle
Any change in temperature, concentration, or pressure on an equilibrium system is called a stress. Le Châtelier’s Principle explains how a system at equilibrium responds to relieve any stress on the system.

14. Le Châtelier’s Principle
The following are several types of stress and how equilibrium shifts to relieve them.
If the concentration of a substance decreases, the reaction that produces that substance is favored. Initially the reverse reaction will take will take place faster than the forward reaction and the system is said to be shifting to the left. (toward the reactant side)
4NH3 + 5O2  4NO + 6H2O + heat
Stress: Less NH3 --The effect on concentration is above.
Concentration changes: If the concentration of one substance is increased, the reaction that reduces the amount of the added substance is favored. Initially the forward reaction will take place faster than the reverse reaction and the system is said to be shifting to the right.
Stress: More NH3 –The effect on concentration is above.

15. Le Châtelier’s Principle
Temperature Changes:
If the temperature is raised, the rates of both the forward and reverse reactions are increased, but not equally. The reverse reaction is endothermic and will absorb some of the applied heat. The endothermic reverse reaction is favored over the exothermic forward reaction.
More reactants will form when temperature is increased and favoring the endothermic reaction. 4NH3 + 5O2  4NO + 6H2O + heat
When temperature is decreased more products will form and the exothermic reaction will be favored.
4NH3 + 5O2  4NO + 6H2O + heat

16. Le Châtelier’s Principle
Pressure Changes
Remember that changes in pressure do not have an effect on the rate of reaction when solids and liquids are involved, however they have an effect on gases.
The following occurs when there are gaseous molecules on both the reactant and product side.
An increase in pressure will favor the reaction toward the side with fewer gas molecules, (LESS NUMBER OF MOLES)
A decrease in pressure will favor the reaction toward the side with the greater number of gas molecules.
When there are the same number of gaseous molecules on both sides pressure changes have no effect on the system.

17. Le Châtelier’s Principle
The addition of a catalyst changes the rates of both the forward and reverse reactions equally. It may cause equilibrium to be established more quickly but does not change any of the equilibrium concentrations.

18. What is the common ion effect
. What is the common ion effect? How does Le Chatelier’s principle explain it?
The common-ion effect is a term used to describe the effect on a solution of two dissolved solutes that contain the same ion.
Common ion effect refers to product of solubility. it's when you ADD a compound in a solution that contains already 1 of the ions of the salt:

19. AgNO3 and NaCl will produce a precipitate of AgCl.
EXAMPLE
AgCl (s) -> Ag+ + Cl-
AgNO3 and NaCl will produce a precipitate of AgCl.
Lead(II) chloride is sparingly soluble in water, and this equilibrium is set up between the solid and its ions in solution:
PbCl2 (s) <-> Pb2+ (aq) + 2 Cl1- (aq)

20. Explain how the solubility of saturated solution of MgCO3 decreases by adding K2CO3

21. Entropy and Enthalpy
The factors that cause chemical and physical changes to occur are two fundamental tendencies in nature that help determine whether or not these changes will occur follow:
Enthalpy: A tendency in nature to change to a state of lower energy. Exothermic reactions will move toward a lower energy state because some of the energy contained in the reactants is released.
Entropy: A tendency in nature to change to a state of greater randomness or disorder. They move from solid (low entropy) to gas (highest entropy).

22. The Equilibrium Expression
The mathematical expression that shows the relationship of reactants and products in a system is called the equilibrium expression.
Example: Write an equilibrium expression for the equilibrium system of nitrogen, hydrogen, and ammonia.
N2 + 3H2  2NH3 + heat
[NH3]2
Keq = ___________
[H2]3[N2]