1. Energy Unit #3

2. What is Energy?

3. A burning match releases energy. Source: ElektraVision/ PictureQuest

4. A Hindu firewalking ceremony in the Figi Islands. Could you do this? Source: Jack Fields/Photo Researchers, Inc.

5. A voodoo lily Source: Neil Lucus/Nature Picture Library

6. Energy Notes Energy –Capacity to do work or produce heat –Capacity to move or change matter

7. Energy Notes Work Examples Moving an object over a distance against a resisting force –Energy stored in the organized motion of molecules A car traveling down the street A train moving down the tracks Pushing a book across the desk

8. Types of Energy Stored –Energy of position (water wheel, book on desk) –Chemical energy (gas, food, batteries) Motion –Mechanical energy (moving parts of machines) Radiant Thermal energy (Sun’s heat) Light Sound: vibration of molecules Potential Kinetic

9. Energy Notes Law of Conservation of Energy In any chemical or physical process, energy is neither created nor destroyed. –Different forms of energy are equivalent. A particular amount of one type of energy can be converted into an exactly amount of another type of energy.

10. Energy Measurement Joule

11. Energy Notes Unit: Conversion (c to J) Metric = joule (J) US = calorie (c) –1 calorie is the amount of heat needed to raise 1 g of H 2 O by 1 °C –1000cal = 1Cal = 1 kilocalorie = food Calories 4.184 J = 1 cal

12. Energy Notes Example –A student uses 30 J of energy putting books on the shelf in the classroom. How many calories of energy did the student exert? –A student eats an entire bag of plan popcorn which contains 60.1 Calories. How many Joules of energy is this?

13. Heat and Temperature

14. Figure 3.12: Equal masses of hot water and cold water separated by a thin metal wall in an insulated box. Is anything going to happen?

15. Figure 3.13: The H 2 O molecules in hot water have much greater random motions than the H 2 O molecules in cold water.

16. Figure 3.14: The water samples now have the same temperature (50°C) and have the same random motions.

17. Heat and Temperature Heat Examples Energy transferred from one body to another due to a temperature difference. –Energy stored in the random motion of molecules Sunlight heating the earth Hot plate with beaker of water

18. Heat and Temperature Exothermic Endothermic System that releases energy into its surroundings Release energy because a change has occurred Combustion reactions System that takes energy in as heat from the surroundings Need energy from outside source in order for a change to occur Phase change – boil water

19. Endo vs. Exo Why are these types of reactions useful? What are some examples in your daily life?

20. Temperature 3 scales Measure of the average kinetic energy of the particles in a sample of matter. Farhenheit (ºF) Celcius (ºC) Kelvin (K)

21. Temperature Converting between ºC and K Example Practice ºC = K – 273 K = ºC + 273 Normal human body temperature is 37 ºC. What is your temperature in K? Surgical instruments must be sterilized at 170 ºC. What is this in K?

22. Temperature Converting between ºC and ºF Example Practice ºC = 5/9(ºF – 32) ºF = 9/5 ºC + 32 It is 100 ºF outside. What temperature is this in ºC? The boiling point of methanol is - 164 ºC. What is the boiling point is ºF?

23. Specific Heat and Calorimetry

24. Specific Heat What this means amount of heat that can be absorbed by 1 gram of material when its temperature increases by 1 o C; unit = J/g o C What bench would you rather sit on, wood or iron, in the summer in AZ? Why?

25. Specific Heat Which holds more heat when exposed to 120 o F sunlight -- a wood or an iron bench (both at the same temperature)? Compare the specific heat capacities. Iron 0.448 J/g o C, wood 1.76 J/g o C The wood bench holds onto more heat so it does not transfer as much to you.

26. Specific Heat and Calorimetry Calorimetry Calorimeter Measurement of the amount of energy released or absorbed during a chemical reaction Device used to measure the transfer of energy to water

27. Complex Calorimeter

28. Simple Calorimeter Test Tube Stirring Rod Thermometer Reaction Water Sealed Container

29. Endo vs. Exo Endothermic- reaction absorbs energy temperature of the surrounding water goes down Exothermic - reaction gives off energy temperature of the surrounding water goes up Energy

30. How does the Heat Flow and How do you Know?

32. Three factors determine the amount of energy (Q) transferred to or from the water. Q= mC p  T 1.Mass of the water in the calorimeter (units = grams) 2.Specific Heat of water 3. Change in the water’s temperature.  T = T final - T initial (units = ºC)

33. Q= mC p  T Example 1 Practice 1 How many calories must be added to 5000 g of water to change it temperature from 20 to 30ºC? How many calories are needed to increase the temperature of 150.0 grams of water from 40.0 to 65.0ºC? specific heat for water

34. Q= mC p  T Example 2 Practice 2 A 2.0 x10 4 grams sample of water has its temperature raised by 3ºC. How many Joules of energy was produced? What is the number of Joules needed to increase the temperature of 50.0 grams of water 15.0ºC? specific heat for water

35. Q= mC p  T Example 3 Practice 3 If 500.0 g of water at 25ºC loses 2500 calories, what will be the final temperature? What is the final temperature after 80.0 calories is absorbed by 10.0 grams of water at 25ºC? specific heat for water

36. Q= mC p  T Example 3 Practice 3 What temperature change,in Celsius, is produced when 6.0 x10 2 grams of water gives off 9.60 kilocalories? What is the change in temperature when 640 calories is given off by 40 grams of water? specific heat for water

37. Q= mC p  T Example 4 Practice 4 If 500.0 g of water at 25ºC loses 2500 calories, what will be the final temperature? What is the final temperature after 80.0 calories is absorbed by 10.0 grams of water at 25ºC? specific heat for water

38. Q= mC p  T Example 5 Practice 5 What is the specific heat of lead if a 30.0 g piece of lead undergoes a 250ºC change while absorbing 229.5 calories? What is the specific heat of an unknown substance if the addition of 950 J of heat energy caused a 20 gram sample to warm from 18ºC to 42ºC?

39. Q= mC p  T Example 6 Practice 6 A quantity of water is heated from 25.0ºC to 36.4ºC by absorbing 325 calories. What is the mass of the water? What is the mass of a piece of copper that undergoes a 25.0ºC temperature change when it absorbs 755 J of energy? Copper has a specific of

40. PreLab: Energy Content in Foods Time to get your lab books ready for Lab! Use the lab handout to help you complete all of the following according to the grading rubric. 1.Title 2.Purpose 3.Background information 4.Materials 5.Procedure and safety 6.Set up data table

41. Class Results GroupPeanut J/g Potato Chip J/g Popcorn J/g Marshmallow J/g 1 2 3 4 5 6 7 8 Ave.

42. Class Results 6 th Period GroupPeanut J/g Cashew J/g Popcorn J/g Marshmallow J/g 1 2 3 4 5 6 7 8 Ave.16,50011,3006872830

43. Review Lab- Energy Content in Foods 5.Food energy is expressed in Calories. 4.184 kJ in 1.000 Calories. Based on the class average for peanuts, calculate the number of calories in a 50.0 g package. 6.Product labels. Determine a serving size and use the class average to calculate the number of calories present in a single serving. Compare your results to the nutritional information.

44. Review Lab- Energy Content in Foods 1.What are 2 possible sources of error? What could be done to reduce these errors? 2.How does calorimetry make use of the law of conservation of energy? 3.What generalization can you make about the relative energy content of fats and carbohydrates?

45. Product Labels 16 oz = 453.59 g Peanuts – 1 oz, 180 Calories Cashews – 1 oz, 160 Calories Popcorn – 1 cup popped, 25 Calories (7g~1 cup) Marshmallow – 30 g, 100 Calories