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(1)CHEMISTRY(1'2)&2856(68&&(66:. HHDW TUDQVIHU SE.

(2) Chemistry End-of-Course Success Copyright Copyright © Texas Education Agency, 2011. The following materials are copyrighted © and trademarked ™ as the property of the Texas Education Agency and may not be reproduced without the express written permission of the Texas Education Agency, except under the following conditions: 1) Texas public school districts, charter schools, and Education Service Centers may reproduce and use copies of the Materials and Related Materials for the districts’ and schools’ educational use without obtaining permission from the Texas Education Agency; 2) Residents of the state of Texas may reproduce and use copies of the Materials and Related Materials for individual personal use only without obtaining written permission of the Texas Education Agency; 3) Any portion reproduced must be reproduced in its entirety and remain unedited, unaltered, and unchanged in any way; 4) No monetary charge can be made for the reproduced materials or any document containing them; however, a reasonable charge to cover only the cost of reproduction and distribution may be charged. Private entities or persons located in Texas that are not Texas public school districts or Texas charter schools or any entity, whether public or private, educational or noneducational, located outside the state of Texas MUST obtain written approval from the Texas Education Agency and will be required to enter into a license agreement that may involve the payment of a licensing fee or a royalty fee. For more information, contact: Office of Copyrights, Trademarks, License Agreements, and Royalties. Texas Education Agency. 1701 N. Congress Ave., Austin, TX 78701-1494; phone 512.463.9437; e-mail [email protected].. .

(3) HEAT TRANSFER SE. Heat Transfer Engage Investigate: The 3-Minute Shake 1. From your instructor, obtain the materials that you will use to conduct the investigation. 2. Remove the stopper and use the temperature probe in interface with the CBL 2™ and calculator to find the temperature of the material. Record the temperature in the table below and remove the temperature probe. 3. Cover the cylinder or tube with a stopper and shake continuously for 3 minutes. 4. Remove the stopper from the cylinder and use the temperature probe to find the temperature after shaking. Record it in the table. 5. Measure and record the mass of the material in the cylinder. Material assigned Mass of material (g) Temperature of material before shaking (°C) Temperature of material after shaking (°C) Change in temperature of material after shaking (°C) Change in temperature per gram of material Duration of shaking (s). •. . What change do you observe?.

(4) HEAT TRANSFER SE. Heat Transfer •. What is a reasonable explanation for your observation?. •. How do the sand or copper particles obtain energy to move?. •. How does the law of conservation of energy apply in this situation?. •. How do you think the temperature would change if you shook the shaker for longer periods of time? Explain.. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(5) HEAT TRANSFER SE. Heat Transfer Explore/Explain 1 Investigate: Hot and Cold Mixture It is common knowledge that when you mix hot and cold water, you get warm water. In this computer simulation, you will explore the quantitative relationships of the heat exchange that occurs when hot and cold water are mixed. 1. Conduct your investigation as required by the computer simulation. 2. Select the amount of hot and cold water to create 1,000 g of warm water. 3. Use mass increments of 1.0 X 102 g, (for example, 2.0 X 102 g of hot water and 8.0 X 102 g of cold water) to make a total of 1.0 X 103 g of warm water. 4. Write down the masses of hot and cold water used to make the mixture, and the initial temperatures in the appropriate column of the data table. 5. Record the final temperature of the mixture and calculate the change in temperature of the hot and cold water. 6. Perform about five trials and complete the data table. 7. Find a relation between the mass and change in temperature of the cold water and the mass and change in temperature of the hot water. Show your calculations, if any, in the space provided. 8. Discuss your observations and analysis questions with your group before writing down your responses. 9. After class discussion of Part I, repeat the same procedure with Part II of the simulation.. .

(6) HEAT TRANSFER SE. Heat Transfer. 1000. 1000. 900. 900. 800. 800. 700. 700. 600. 600. 500. 500. 400. 400. 300. 300. 200. 200. 100. 100. Temperature = 0 °C. Temperature = 100 °C. 1000 900 800 700 600 500 400 300 200 100. Mixture Mass = 1.0 X 103 g Temperature = ? °C. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(7) HEAT TRANSFER SE. Heat Transfer Observations Part I Initial temperature of the hot water = Initial temperature of the cold water = WARM MIX Final temperature (°C). Calculations. . HOT WATER Mass of hot water (g). Change in temperature (°C). COLD WATER Mass of cold water (g). Change in temperature (°C).

(8) HEAT TRANSFER SE. Heat Transfer Part II Initial temperature of hot Liquid X = Initial temperature of the cold water = WARM MIX Final temperature (°C). HOT LIQUID X Mass of hot liquid (g). Change in temperature (°C). COLD WATER Mass of cold water (g). Change in temperature (°C). Calculations. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(9) HEAT TRANSFER SE. Heat Transfer Analysis and Conclusions Part I 1. What did you observe about the final temperature of the mixture when you mixed different quantities of hot and cold water?. 2. Describe the energy conservation equation for this heat exchange.. 3. What mathematical relation do you observe between the mass and change in temperature of the hot water when compared with the mass and change in temperature of the cold water?. 4. Based on the mathematical relation observed, what is the final temperature of the mixture when 2.0 X 102 g of water at 80 °C is mixed with 4.0 X 102 g of water at 10 °C?. .

(10) HEAT TRANSFER SE. Heat Transfer Analysis and Conclusions Part II 5. What did you observe about the final temperature of the mixture when you mixed different quantities of hot Liquid X and cold water?. 6. Describe the energy conservation equation for this change.. 7. What mathematical relation do you observe between the mass and change in temperature of hot Liquid X when compared with the mass and change in temperature of the cold water?. 8. Based on the mathematical relation observed, what is the final temperature of the mixture when 2.0 X 102 g of Liquid X at 80 °C is mixed with 4.0 X 102 g of water at 10 °C?. 9. Based on your observations from Part I and Part II, explain why the conservation of energy equation was different.. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(11) HEAT TRANSFER SE. Heat Transfer Notes:. .

(12) HEAT TRANSFER SE. Heat Transfer Application: Hot and Cold Mixture In the mixtures below, calculate the required item. Show all your work. Component 1. Component 2. Mixture. Material = Solid Mass = 100.0 g Specific heat = 0.46 J/g °C Temperature = 100. °C. Material = Water Mass = 200.0 g Specific heat = 4.184 J/g °C Temperature = 25. °C. Final temperature = ___?___. Material = Olive oil Mass = 100.0 g Specific heat = 2.0 J/g °C Temperature = 80. °C. Material = Olive oil Mass = 200.0 g Specific heat = 2.0 J/g °C Temperature = ___?___. Final temperature = 33. °C. Material = Metal Mass = 56.0 g Specific heat = ___?___ Temperature = 100 °C. Material = Water Mass = 100.0 g Specific heat = 4.184 J/g °C Temperature = 25 °C. Final temperature = 27 °C. 1. 2. 3. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(13) HEAT TRANSFER SE. Heat Transfer Explore/Explain 2 Design: Specific Heat Which metal has the highest specific heat? How would you find the specific heat of the given metals? Plan your experiment with your team. Write your notes in the space below. (diagrams allowed). .

(14) HEAT TRANSFER SE. Heat Transfer Investigate: Specific Heat After class discussion, write down any changes in your original experimental plan in the space below.. Safety Study the procedure that you will follow. Discuss safety precautions that must be used and list them in the box space below.. Data. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(15) HEAT TRANSFER SE. Heat Transfer Calculations. Results. Analysis and Conclusions 1. List the metals used in this investigation in order, from highest specific heat to lowest specific heat.. 2. If the same amount of heat was provided to the same mass of the five metals, which metal would have the highest temperature? Why?. .

(16) HEAT TRANSFER SE. Heat Transfer 3. If the same amount of heat was provided to the same mass of the five metals, which metal would have the lowest temperature? Why?. 4. Is specific heat capacity an intensive or extensive property? Why?. 5. How is specific heat similar to density?. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .


(18) HEAT TRANSFER SE. Heat Transfer Application: Specific Heat Answer the following questions. Show all your logic and your work. 1. A metal wire with a mass of 55.0 g is heated from 19.0 °C to 86.0 °C. The wire uses 1,435 J of electrical energy. What is the specific heat of the metal?. 2. A 100. g strip of alloy containing iron and copper in equal amounts is placed in a burner that supplies 4.0 kJ of heat. If the initial temperature of the alloy is 20.0 °C, what is the final temperature of the alloy? (Cp for iron is 0.460 J/g °C. Cp for copper is 0.385 J/g °C.). © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(19) HEAT TRANSFER SE. Heat Transfer Explore/Explain 3 Design: Heat of Fusion How much heat would it take to melt 1 g of ice? Plan your experiment with your team. Write your notes in the space below. (diagrams allowed). .

(20) HEAT TRANSFER SE. Heat Transfer Investigate: Heat of Fusion Write down any changes in your original experimental plan in the space below.. Safety Study the procedure that you will follow. Discuss safety precautions that must be used and list them in the box space below.. Data. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(21) HEAT TRANSFER SE. Heat Transfer Calculations. Results. Analysis and Conclusions 1. What is the heat conservation equation for the melting of ice in this investigation?. 2. How does the temperature change during melting? Why?. .

(22) HEAT TRANSFER SE. Heat Transfer 3. Why is it important to have unmelted ice in the cup that is removed at the end of the data collection?. 4. How much heat would it take to melt 1.00 mole of ice? (show calculation). © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .


(24) HEAT TRANSFER SE. Heat Transfer Application: Heat of Fusion and Heat of Vaporization Answer the questions below. Show all your work. 1. 4.35 kJ of heat is applied to 50.0 g of ice at 0 °C. What is the mass of the remaining ice?. 2. How much heat in joules would it take to transform 100.0 g of ice at 0 °C into vapor at the boiling temperature of 100.0 °C?. 3. How much heat is released when 5.00 kg of water at freezing temperature freezes to solid ice?. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(25) HEAT TRANSFER SE. Heat Transfer Elaborate Investigate 1: Heat Transfer in the Real World Health Normal human body temperature is 37.0 °C on average. When a person is sick, the body temperature increases above the normal temperature. Elevated body temperatures can cause considerable harm to body systems, especially in infants and young children. Placing the sick person or child in a cool-water bath for a short time to lower the body temperature is often recommended. This procedure has to be performed very carefully when working with young children to prevent drowning. The volume of water used for the bath is controlled so that the child’s face remains above the water. The temperature of the water is also monitored carefully so that it is not more than 10 °C below the body temperature of the sick person to avoid cold shock to the body. A child with a body mass of 11.0 kg has a temperature of 39.5 °C. The volume of water is restricted to 10.0 L to allow the child’s face to remain above the water. What should the temperature of the water be to lower the child’s temperature to 37.0 °C? (specific heat capacity of the human body is 3.470 J/g °C). .

(26) HEAT TRANSFER SE. Heat Transfer Elaborate Investigate 2: Heat Transfer in the Real World Home A great deal of energy is required to heat swimming-pool water. The operating costs of a pool may be greatly reduced through simple changes to the pool maintenance and the use of more efficient and environmentally friendly heat sources. A home in a Texas town has a standard-sized pool with dimensions of 4.2 m by 8.4 m and a depth of 1.8 m. The average temperature in the region during November is 20.0 °C. The temperature of the heated pool is set at 26.0 °C, and the pool is operated for 4.0 hours each day. The cost of heating the pool for that month is $250.00. How much money could be saved during that month if the pool temperature was lowered to 23.0 °C? (Assume that the swimming pool contains pure water.). © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

(27) HEAT TRANSFER SE. Heat Transfer Evaluate Answer the following questions. Show all your logic and your work. 1. Using the chemistry reference tables, calculate the amount of heat energy required to convert 100.0 g of ice at –20.0 °C to steam at 120.0 °C as shown in the diagram below.. Temperature °C. 120.0 °C. –20.0 °C Heat Energy. .

(28) HEAT TRANSFER SE. Heat Transfer 2. Using the calorimetric information shown below, calculate the specific heat of the metal.. Mass of water = 50.0 g Initial temperature of water = 20.0 °C Mass of metal = 10.0 g Initial temperature of metal = 100.0 °C. Final temperature of water and metal = 21.5 °C. © 2011 TEXAS EDUCATION AGENCY. ALL RIGHTS RESERVED.. .

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