1. Chemical Kinetics and Equilibrium

2. Standards: Reaction Rates
8a. rate of reaction is the decrease in concentration of reactants or the increase in concentration of products with time.
8b. reaction rates depend on such factors as concentration, temperature, and pressure.
8c. the role a catalyst plays in increasing the reaction rate.

3. REVIEW: Parts of a chemical reaction
Reaction #1: A + B  AB
Reactants
Product
Reaction #2: 2A + B  A2B
Coefficient
Subscript

4. Creating a Model of a Chemical Reaction
Sketch of what is happening on a molecular model of a chemical reaction (use circles to represent atoms and label each one, make sure to show which atoms are bonded)
NaCl (s)  Na+ (aq) + Cl- (aq)  + Cl Na Cl
Have some colored salts and solutions to mix Na  + B A B A

5. Direction: Using the balanced equation below, create a molecular model of this chemical reaction (use circles for atoms, show bonds and label each atom)
Mg + 2HCl  MgCl2 + H2 + 2

6. In Class Activity: POGIL 1
In Class Activity: POGIL 1. Read the scenarios about the collision theory 2. Answer the worksheet.

7. Collision Theory: reactants forming products using energy and proper orientation

8. A B Describe the difference between the two graphs.
Which graph shows a spontaneous reaction? Which one will have a faster rate? Explain your choice. B

9. Energy Diagram
*Reaction needs to surpass activation energy (Ea) to turn the reactants to products. * The middle steps of any reaction is called the transition state.
Exothermic
Endothermic

10. REAGENTS  PRODUCTS
What can we conclude from this graph? What does the slope of of the line represent?
Rate of reaction-- decrease in [reactants] or the increase [products] over time.

11. What are the factors that determines the rate of reaction?

12. Explain how reaction rates depend on such factors as concentration, temperature, and pressure (use the pictures below to support your argument)
Pressure affects the rate of reaction, especially when you look at gases. When you increase the pressure, the molecules have less space in which they can move. That greater density of molecules increases the number of collisions
When you raise the temperature of a system, the molecules bounce around a lot more because they have more energy. When they bounce around more, they are more likely to collide.
If there is more of a substance in a system, there is a greater chance that molecules will collide and speed up the rate of the reaction. If there is less of something, there will be fewer collisions and the reaction will probably happen at a slower speed.
Low Pressure
High
Pressure

13. -- the frequency of collisions between reactants
Catalysts
the frequency of collisions between reactants
-- rearrange the orientation of reactants
-- speeds up reaction, not consumed
Ex. biological enzymes, catalase etc.
--reducing intramolecular bonding within reactant molecules, or donating electron density to the reactants.

14. TED ED VIDEO: Chemical Reactions

16. What conclusions can we draw from this demonstration?
Kinetics Lab Part I: Using Visual Clues to indicate the rate of a chemical reaction
C6H12O6 in NaOH + Indicator+ O Indicator oxidized + Products
What conclusions can we draw from this demonstration?
Kinetics Lab Part II: Graphing rate of reaction of a combustion reaction
C20H42 + O2  CO2 + H2O + energy (heat and light) Conclusion: *After plotting the graph, describe the relationship of your product vs. reactant *What conclusions can you draw from your data about the rate of this combustion reaction.

17. Rate Order of Reaction – how the amount of reactant affects how fast the reaction
Zero Order
1st Order
2nd Order
Formula
Rate = k x 0
If the concentration of reactant [x] doubles the rate….

18. Rate Order of Reaction – how the amount of reactant affects how fast the reaction
Zero Order
1st Order
2nd Order
Formula
Rate = k x 0
Rate = k x 1
Rate = k x 2
If the concentration of reactant [x] doubles the rate….
--will remain the same
-- will double
-- will quadruple

19. What conclusions can we draw from this demonstration?
Kinetics Lab Part I: Using Visual Clues to indicate the rate of a chemical reaction
C6H12O6 + NaOH+ Indicator+ O Indicator oxidized [BLUE]
[CLEAR]
What conclusions can we draw from this demonstration?
Kinetics Lab Part II: Graphing rate of reaction of a combustion reaction
C20H42 + O2  CO2 + H2O + energy (heat and light) After plotting the graph, describe the relationship of your product vs. reactant What conclusions can you draw from your data about the rate of this combustion reaction.

20. Standards: Equilibrium
9a. Students know how to use Le Chatelier's principle to predict the effect of changes in concentration, temperature, and pressure.
9b. Students know equilibrium is established when forward and reverse reaction rates are equal.
9c. Students know how to write and calculate an equilibrium constant expression for a reaction.

21. What can we conclude from each chart?
Based on these 2 charts, define what it means to be
be in equilibrium? B

22. Equilibrium when forward and reverse reaction rates are equal and the concentration of reactants and products eventually remain constant

23. H2 + F2 2HF Which reaction is in equilibrium? Explain why.
HCl + NaOH H2O + NaCl

24. Disturbance # 1. Add more products (change concentration)
A + B+ Heat A-B
Disturbance # 1. Add more products (change concentration)

25. Disturbance # 2. Add more heat to this endothermic reaction
A + B+ Heat A-B
Disturbance # 2. Add more heat to this endothermic reaction

26. A (g)+ B(g)+ Heat A-B(g)
Disturbance # 3.
Increase the pressure in the container that contains this reaction

27. Le Chatelier’s Principle
In a reversible chemical reaction, when stress is applied to a system in an equilibrium, the reaction will shift in a direction that relieves the stress and a new equilibrium will be established. Stress: Changing Concentration Pressure Temperature

28. Equilibrium Activity Q: endothermic or exothermic?
A + B+ Heat A-B
Q: endothermic or exothermic?
Q: What happens if we add heat? If
we cool it down

29. Quiz: Chp. 16 Kinetics and Equilibrium
1. Draw and explain Collision Theory 2. What are the 5 factors that can affect kinetics/reaction rate/ rate order 3. Predict direction of reaction if temp./pressure/concentration changes 4. Parts of an energy diagram and determine if the reaction will occur 5. Predicting which side of the equation is favored based on Keq and which direction will the reaction happen 6. Labs: **Transferring Water with Straws (what is the analogy) **Blue Bottle demonstration and melting candle 7. Reading Graphs: Equilibrium graph AND Reaction Rate
VOCABULARY
*Le Chatelier’s Principle *Transition State * Collision Theory
*Equilibrium *Forward vs * Endo vs. Exothermic
*Activation Energy (Ea) Reverse Reaction *Catalyst