2. Catalyst Look over your learning logs What are the three learning targets that you think will be the hardest for you? Copy them down. Why do you think that? End

3. Top Achievers (>80%) Period 1 Ana Hidalgo Sindi Vazquez Trent Nettles Martha Nochez Jonathan Flores Daisy Benitez Giorgi Trujillo Alexis Valle Eric Cano

4. Top Achievers (>80%) Period 6 Henry Rodriguez Luis Garcia Maria Servera

5. Top Achievers (>70%) Period 3 Camden Tillman

6. Top Achievers (>70%) Period 4 Ricardo Interiano Mike Davalos Breidy Rodriguez Melissa Rodriguez

7. Top Achievers (>70%) Period 2 Noe Bonfil Armando Raya Genesis Acajabon

8. Biggest Growth (>15% Growth) Period 3 Jasmine Dillard Camden Tillman Leslie Diaz Jesus Rubio

9. Biggest Growth (>15% Growth) Period 1 Ilynn Perez Giorgi Trujillo Josue Bravo

10. Biggest Growth (>15% Growth) Period 6 Maria Servera

11. Biggest Growth (>15% Growth) Period 4 Melissa Rodriguez Elizabeth Ayala

12. Biggest Growth (>15% Growth) Period 2 Genesis Acajabon Leslie Martinez Valencia Alamilla Marlene De La Torre Monae Warthen Mysty Carpenter Rashaun Hicks

14. McDonald’s French Fries Reading Read the article with your group. Answer the questions and be prepared to discuss with the class.

15. Reading Debrief What is decomposition? Why don’t McDonalds fries or burgers decompose? How can we slow the rate at which something decomposes? Should we be adding chemicals to our foods in order to preserve them? What other questions did you have during this reading?

16. Catalyst What is decomposition? Why don’t McDonalds fries or burgers decompose? How can we slow the rate at which something decomposes? Should we be adding chemicals to our foods in order to preserve them? End

17. Unit 8 – What is McDonald’s Putting In Its French Fries?

18. ACS Chemistry Olympiad Old Tests! Let me get somma dat! Mr. Astor’s File Cabinet – Week of March 3, 2014

19. LECTURE 8.1 – FACTORS ON RATE OF REACTION

20. Today’s Learning Target LT 8.1 – I can describe the rate of a reaction using the ideas of concentration of reactants, concentration of products, and time. I can explain why rate is dependent on concentration. LT 8.2 – I can calculate the average rate of reaction with respect to the reactants and/or products. LT 8.3 – I can hypothesize about the impact that concentration, temperature, and pressure have on the rate of a chemical reaction.

21. Today’s Focus Question What is the typical rate at which food decomposes?

23. How are rates measured?

24. I. Rate of Reaction A rate describes how fast something changes with time. Rate is measured either by the rate of formation of product or the rate of disappearance of the reactants.

25. How is collision theory related to rates?

26. I. Collision Theory Reactions occur when molecules collide. Therefore, more collisions, a faster overall rate of reaction. Less collisions, a slower rate.

27. SUMMARIZE Use the following terms: Rates Collision Formation Disappearance

28. What are ways to impact the rate of reaction?

29. I. Concentration, Temperature, Pressure, and Rate As concentration, the rate also increases As temperature, the rate also increases. As pressure, the rate also increases. This is due to the increased amount of collisions

30. What determines the rate of a reaction?

31. I. Concentration and Rate As you increase the concentration, the rate of reaction increases. The higher the concentration the more collisions that are occurring, which increases the rate.

32. II. Temperature and Rate As you heat up molecules they begin to move faster. The faster molecules move the more they collide, which means a faster rate.

33. III. Pressure and Rate As you increase the pressure molecules collide more into the wall of the container and into each other. Therefore, as you increase pressure, you increase the rate of the reaction.

34. Summarize Use the following words: Pressure Temperature Concentration Rate Collisions

35. White Board Questions H 2 + Cl 2  2HCl The rate can be described as the decrease of _____ with time H 2 + O 2  H 2 O The rate can be described as the increase of _____ with time NaOH + HCl  H 2 O + NaCl The rate can be described as the decrease of _______ with time

36. White Board Questions H 2 + Cl 2  2HCl If I increase the concentration of H 2, how will the rate change? If I decrease the pressure, how will the rate change? I heat the container, how will the rate be changed? I decrease the amount of Cl 2, how will the rate change?

37. White Board Questions C 6 H 6 + Br 2  C 6 H 5 Br + HBr Which of the following changes will cause an increase in the rate of the above reaction? A. Increasing the concentration of Br 2 B. Decreasing the concentration of C 6 H 6. C. Increasing the concentration of HBr D. Decreasing the temperature

38. White Board Questions I run the reaction: C 6 H 12 O 6 + 6 O 2  6 CO 2 + 6 H 2 O If I begin with 0.25 M O 2 and after 100 seconds the concentration is 0.12 M, then what is the rate of this reaction? I run the same reaction and I begin with 0 M CO 2 and after 232 seconds the concentration of CO 2 is 0.75 M.

39. Lab – Alka Seltzer Rockets Read and annotate the procedure for the lab

40. Lab Logistics You will be working in groups of 4 Decide who will take on each role, or let one person do all of the items below: (1) Dropper and Capper (drops in tablet, caps it, and turns it upside down) (2) Filmer (3) Cup Placer (places cup over test tube) (4) Timer/measurer

41. LAB DEMONSTRATION

42. Expectations Explain the influence of (1) concentration and (2) temperature influence the rate of a reaction of Alka Seltzer. You will turn in 1 COPY PER GROUP of your findings and post-lab questions at the end of class.

43. Lab Work Time

44. Post-Lab Analysis

45. Exit Ticket 1.If you increase the pressure of a container, how is the rate of the reaction impacted? 2.What is collision theory and how is it related to rates? 3.I run the reaction: C 6 H 12 O 6 + 6 O 2  6 CO 2 + 6 H 2 O If I begin with 0.25 M O 2 and after 100 seconds the concentration is 0.12 M, then what is the rate of this reaction?

46. College-Ready Question: 2CO + O2  2CO2 If the above reaction takes place inside a sealed reaction chamber, then which of these procedures will cause a decrease in the rate of reaction? A raising the temperature of the reaction chamber B increasing the volume inside the reaction chamber C removing the CO2 as it is formed D adding more CO to the reaction chamber

48. Closing Time Turn in the lab questions as you leave. Work on your lab report!