Thermodynamics

Documents you may need:

Passive Solar Homes Article (google doc) and Questions (google doc) (This is Activity #18 and needs to be completed in your Notebook)

Dipping (Drinking) Bird Lab (pdf or google doc) If you were absent, watch this video and complete the lab. (This is Activity #21 and needs to be completed in your Notebook)

Ch. 12 Study Guide worksheet (pdf or google doc) and Answers (to the front side) (Answers)

Freezing Point Lab (pdf or google doc)

Heat Stations Lab (pdf or google doc)

Discussion Topics with notes from our review day (pdf)

Heat Devices Practice Problems (with partial solutions) (pdf)

Lecture Notes: (You will need to be signed in to your PUSD Google account to access them)

Laws of Thermodynamics (This is Activity #19 and needs to be completed in your Notebook)

Heat Devices (This is Activity #20 and needs to be completed in your Notebook)

Thermodynamics (These are just for reference)

Graphs & Heat of Fusion and Vaporization (These are just for reference)

Homework Help:

February 4th, 2016: Solutions to Pg. 336 #56, 57, & 64

Solutions are HERE

February 5th, 2016: Homework Packet List

1. Pg. 322 #10-12, 14, 15; Pg. 336 #38-40

2. Pg. 331 #27, pg. 336 #53, 54, 58, 61, 62

3. Pg. 331 #28, 29; pg. 336 #55, 63, 69

4. Pg. 336+ #56, 57, 64

5. Pg. 336 #41-43, 45-50

6. Ch. 12 Study Guide

7. DWQs (8)

January 29th, 2016: Pg. 331 #27; Pg. 336+ #53, 54, 58, 61, 62

53. Don't forget to convert to kilograms! Use Q=mC(delta)T and solve for C. (~1000)

54. Don't forget to convert to kilograms! Use Q=mC(delta)T and solve for Q (>20,000)

58. Given this amount of energy, solve for the mass of the water that could be heated with than energy change. Then given the fact that the density of water is 1 kg/L you can solve for the liter. (<1)

61. Given the mass and the heat of Fusion to solve for the heat absorbed. (<7E6)

February 1st, 2016: pg. 331 #28, 29; pg. 336 #55, 63, 69

28. Three steps: 1. Calculate the heat needed increase the temperature from 80 to 100 degrees using Q=mC(delta)T. (>4000) 2. Calculate the heat needed to vaporize that much liquid. (>1.1E5) 3. Calculate the heat needed increase the temperature from 100 to 110 degrees using Q=mC(delta)T. (>1000) LAST STEP: add it all up. (<1.2E5)

29. Two steps: 1. Calculate the heat needed increase the temptrature from 10 to 357 degrees using Q=mC(delta)T. (>5E4) 2. Calculate the heat needed to vaporize that much liquid. (<3.1E5) LAST STEP: add it all up. (>3.5E5)

55. The final temperature of both the tungsten and water is 21.6 degrees.Since the heat gained by the water is lost by the tungsten, you can find the amount of energy lost by the water using Q=mC(delta)T. (>1000) Set this equal to the mC(delta)T for Tungsten; you know everything but the Specific Heat of Tungsten. (<200)

63. Given the information for the car, find the KE of it. If this much KE is completely absorbed by the brakes, you can find the change in temperature. Since the brakes are iron, look up the specific heat of iron. (<30)

69. Given the information for the car, find the KE of it. If this much KE is completely absorbed by the brakes, you can find the change in temperature. Since the brakes are aluminum, look up the specific heat of Aluminum. (>10)

February 2nd, 2016: pg. 336 #56, 57, 64

56. Similar to the practice problems in class. Since the heat gained by one sample is lost by the other, you can solve for the final temperature they both come to. Try using the equation below. Remember to state that energy is conserved! (>60)

57. Similar to the practice problems in class. Since the heat gained by one sample is lost by the other, you can solve for the final temperature they both come to. Try using the equation below. Remember to state that energy is conserved! (>10)

64. Five step problem: 1. Calculate the heat needed increase the temperature from -200 to 0 degrees using Q=mC(delta)T. (>400) 2.Calculate the heat needed to melt that much ice. (>3000) 3. Calculate the heat needed increase the temperature from 0 to 100 degrees using Q=mC(delta)T. (>4000) 4. Calculate the heat needed to vaporize that much liquid. (>2.2E5) 5. Calculate the heat needed increase the temperature from 100 to 120 degrees using Q=mC(delta)T. (>400) LAST STEP: add it all up. (<3.1E5) Remember that the specific heat for ice which is different than the specific heat for liquid water which is different from the specific heat for steam.

January 28th, 2016: Freezing Point Lab (Stock data) use only if you were absent!