2. Calorimetry

3. Do Now Read the description of Calorimetry in the textbook on page 523. Answer the following questions: 1. What is calorimetry used for? 2. What is the general set-up of a calorimeter? 3. What data is collected in calorimetry, and what other information is needed in order to calculate the heat absorbed or released?

4. Agenda Do Now10 min. Experimental Design Review5 min. Calorimetry Example 115 min. Calorimetry Calculations15 min. Calorimetry Example 220 min. Calorimetry Example 320 min. Closing5 min.

5. Experimental Design What are the major parts of an experiment to look out for as we read someone else’s summary of their experiment? Aim/Purpose Methods/Tools Indep. Variable Dep. Variable

6. Agenda Do Now10 min. Experimental Design Review5 min. Calorimetry Example 115 min. Calorimetry Calculations15 min. Calorimetry Example 220 min. Calorimetry Example 320 min. Closing5 min.

7. Experimental Design (4 min.) Read the summary of the experiment conducted. Keep a close watch for: 1. Aim 2. Methods 3. Independent Variable: 4. Dependent Variable:

8. Experimental Design 1. Aim 2. Methods 3. Independent Variable 4. Dependent Variable

9. Question 1 According to the data from Figure 1, Figure 2, and Figure 3, which of the brands of chips should produce the largest change in temperature in the beaker filled with 1 kg of water? How do you know?

10. Question 2 According to Table 2, which brand of chip produced the largest change in temperature in the beaker filled with water?

11. Agenda Do Now10 min. Experimental Design Review5 min. Calorimetry Example 115 min. Calorimetry Calculations15 min. Calorimetry Example 220 min. Calorimetry Example 320 min. Closing5 min.

12. Calculations for Calorimetry Q = mCΔT can be used to calculate the amount of heat absorbed or released when you know 1.the mass (m) 2.specific heat (C), and 3.the change in temperature of a system (ΔT). What if you don’t know the specific heat of a substance? Or, what if the substance is a solid and you can’t place thermometer in it?

13. Calorimetry Calorimetry uses water to calculate the heat absorbed or released from a system because the specific heat of water is known, and the temperature and mass of water can be easily measured.

14. Calorimetry So, if after using Q = mCΔT, you calculate that water has absorbed 4,000J of energy in the form of heat…. … What amount of heat energy was released by the Dorito sample?

15. Calculations Brand of Chip Mass of Chip Sample Burned Initial Temperature of the Water ( o C) Final Temperature of the Water ( o C) Lay’s28 g20.5131.5 Takis28 g20.3132.7 Doritos28 g20.7140.7 Let’s do the math together…

16. Answers

17. Question 3 According to your calculations, which brand of chip produced the amount of energy closest to the amount estimated by the nutrition facts on the back of the package?

18. Question 4 Prior to the experiment, the student predicted that the Lay’s brand packaging would have the most accurate nutrition facts. Does the data from this experiment support that prediction? Why or why not?

19. Agenda Do Now10 min. Experimental Design Review5 min. Calorimetry Example 115 min. Calorimetry Calculations20 min. Calorimetry Example 220 min. Calorimetry Example 315 min. Closing5 min.

20. Partner Practice Do the math and answer the questions in pairs.

22. Agenda Do Now10 min. Experimental Design Review5 min. Calorimetry Example 115 min. Calorimetry Calculations15 min. Calorimetry Example 220 min. Calorimetry Example 320 min. Closing5 min.

23. Independent Practice (15 min.) Complete the last Calorimetry experimental set-up example on your own. Answer all questions and complete all calculations.

24. Agenda Do Now10 min. Experimental Design Review5 min. Calorimetry Example 115 min. Calorimetry Calculations15 min. Calorimetry Example 220 min. Calorimetry Example 320 min. Closing5 min.

25. Create Calorimetry Procedures Example for creating own procedures: Find the q per gram of a peanut Find the amount of heat produced per mole of a reaction between baking soda and vinegar If you want to create your own procedure and aim, check with your teacher first. Design a calorimeter to come with 10% error of the true caloric value of a known substance (you must justify the choices/alterations you made to the experimental design in order to make your calorimeter more efficient). 1. Peanuts or other nuts 2. Heavy wire to create a stand for peanuts 3. Some empty cans (soda, juice, coffee, or otherwise) 4. Styrofoam cups and lids (or corrugated cardboard pieces to make lids) 5. Thermometers 6. Stirrers (can be made from the wire as well) 7. Baking soda 8. Vinegar 9. Matches 10. Ring stands 11. Ring clamps 12. Wire mesh 13. Distilled water