CALCULATING THERMAL ENERGY TRANSFER

Only one student has the Wizer open.Both students have calculators. (both students calculate to make sure the answer is correct)Please use scrap paper if needed.No proof of work.Fill in the information below. Who has the Wizer open?Who is the partner? Q = m x ΔT x Cp 1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron. 10350 J .46 J 2.17 J 2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J 297 J 2.97 J 367 J 3. Calculate the heat capacity of a piece of wood if 1500.0 g of the wood absorbs 6.75×104 (67500) joules of heat, and its temperature changes from 32°C to 57°C. 1.8 J 1125 J .56 J 4. 100.0 mL of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4.18 J calculate the amount of heat energy needed to cause this rise in temperature. 789 J 1.3794 J 13794 J 5. 25.0 g of mercury is heated from 25°C to 155°C, and absorbs 455 joules of heat in the process. Calculate the specific heat capacity of mercury. 2366 J 0.14 J 140 J 6. What is the specific heat capacity of silver metal if 55.00 g of the metal absorbs 47.3 J of heat and the temperature rises 15.0°C? 17 J .06 J 12.9 J 7. A 0.3 g of piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by heat to the copper is 66,300 J. If the specific heat of copper is 390 J what is the change of the copper’s temperature? 567 °C 57 °C 861 °C 8. How much energy must be absorbed by 20.0 g of water to increase its temperature from 283.0 °C to 303.0 °C? (Cp of H2O = 4.184 J °C) 1672 J 96 J 1674 J 9. When 15.0 g of steam drops in temperature fro 275.0 °C to 250 °C, how much heat energy is released?(Cp of H2O = 4.184 J °C) -1569 J 1569 J -1568 J 10. How much energy is required to heat 120.0 g of water from 2.0 °C to 24.0 °C? (Cp of H2O = 4.184 J °C) 63 J 11046J 11056 J 11. What is the specific heat of a substance that absorbs 2500 joules of heat when a sample of 100 g of the substance increases in temperature from 10 °C to 70°C? .42 J 4167 J .36 J 12. If 200 grams of water is to be heated from 24.0°C to 100.0°C to make a cup of tea, how much heat must be added? The specific heat of water is 4.18 J 11 J 836 J 63536 J 13. A block of aluminum weighing 140 g is cooled from 98.4°C to 62.2°C with the release of 1080 joules of heat. From this data, calculate the specific heat of aluminum. -0.21 J 0.21 J 0.21 g°C 14. The specific heat of wood is 2.03 J How much heat is needed to convert 550 g of wood at -15.0°C to 10.0°C? -10.8 J 27913 J 6773 J 15. What is the total amount of heat needed to change 2.25 g of silver at 0.0°C to 200.0°C? The specific heat of silver is 0.129 J 11.5 J 5805 J 58.05 J 16. Granite has a specific heat of 800 J What mass of granite is needed to store 150,000 J of heat if the temperature of the granite is to be increased by 15.5°C? 1.21 g .12 g 12.10 g 17. A metal weighing 50.0 g absorbs 20.0 J of heat when its temperature increases by 150.0°C. What is the specific heat of the metal? 0.03 J .003 J 60 J 18. When a 100.0 g nugget of pure gold is heated from 35.0°C to 50.0°C, it absorbed 4000.0 J of energy. Estimate the specific heat capacity of gold. .375 J 2.7 J .81J 19. The specific heat capacity of diamond is 0.5050 J What mass of diamond is needed to change the temperature from 10.5°C to 15.6°C, when 64.4 J of energy is applied to the diamond? 25 g 6.4 g 23 g 20. Ten grams of an unknown substance was heated from 35.0°C to 65.0°C. In this process, the substance absorbed 15000 J of energy. What is the approximate specific heat capacity of the substance? .02 J 50 J 4500 J