Background Heat is determined by: Q = cmT, where c is the specific heat of the m

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Background Heat is determined by: Q = cmT, where c is the specific heat of the material. The specific heat of a material can be determined by using a calorimeter with a known amount of water and by measuring the temperature change. In this lab, you will be determining the specific heat of a metal by measuring the temperature change of water in the calorimeter when heated metal is placed in the water. The amount of heat loss from the metal should equal the amount of heat gained by the water. You will also be examining the heat loss and heat gain relationship with water and determining the latent heat of fusion for ice. For water, c = 4186 J/kgoC. The heat of fusion for ice is 333000 J/kg. Procedure Computer Setup 1. Open the lab file “Heat.cap”. Experimental Setup: Part I – Specific Heat of Metal 1. Determine the mass of the empty calorimeter and record it in the data table (use the corresponding number with the metal you chose). 2. Fill the calorimeter about half full with room temperature water. Determine the new mass and record it in the data table. 3. Fill the steamer about half full with water from the faucet. Place the steamer on a hot plate and begin to heat the water inside. 4. Place about 75-125 g of metal into the metal holder for the steamer. Record the mass of the metal in the data table. 5. Place the metal holder into the steamer and put a temperature sensor in the metal and one in the water in the calorimeter. Performing the Experiment: Part I – Specific Heat of Metal 6. Click “record”. 7. Once the temperature of the metal has reached about 65oC, remove the metal from the steamer using a hot pad and quickly pour it into the water. 8. Stir the contents well with the temperature sensors. 9. When the temperature on the graph levels out and no longer changes much, click stop. Analyzing the Data: Part I – Specific Heat of Metal 10. Use the “zoom select” tool to zoom in on the region of the graph before mixing the metal and the water. Record the temperatures of the metal and water before the mix in the data table. Be careful to note that the axes have different temperature scales. 11. Use the “zoom select” tool to determine the final temperature of the mixture of water and metal after it levels off but before it begins to fall. Record this in the data table as the final temperature. Repeat the Experiment with 1 more metal so you will do 1 trial with 2 different metals. Be sure the metal is dry before starting over and use room temperature water in the calorimeter. Experimental Setup: Part II: Heat Gain/Heat Loss 1. Determine the mass of 2 Styrofoam cups and report their mass in the data table. 2. Add approximately 100 mL of warm water to 1 cup and 100 mL of cold water to the other cup. Reweigh both cups and record their masses in the table. Be sure to keep track of which cup is which. You may want to write which one is which on the cup. 3. Place 1 temperature sensor in each of the cups. Be careful to hold the cups up so they do not spill. Performing the Experiment: Part II: Heat Gain/Heat Loss 1. Click “record”. 2. After a few seconds, pour the cold water into the hot water cup and place both temperature sensors in the cup. 3. Stir the contents well. 4. When the temperature on the graph levels out and no longer changes much, click stop. Analyzing the Data: Part II: Heat Gain/Heat Loss 1. Use the “zoom select” tool to zoom in on the region of the graph before mixing the water. Record the temperatures of the hot and cold water before the mix in the data table. 2. Use the “zoom select” tool to determine the final temperature of the mixture of water after it levels off. Record this in the data table as the final temperature. Computer Setup: Part III - Heat of Fusion In this experiment, you will use the same computer setup you used in the first part. However, you will only be using 1 temperature sensor. You can just ignore the data the other sensor gives you. Experimental Setup: Part III - Heat of Fusion 1. Determine the mass of a dry Styrofoam cup and record it in the data table. 2. Put approximately 100 mL of warm water into the cup and record the new mass in the table. 3. Obtain about 3-4 cubes of ice. Dry the ice with a paper towel. Performing the Experiment: Part III - Heat of Fusion 1. Click “start”. 2. Place the thermometer into the water. 3. Once the temperature levels out, dump the ice into the water. 4. Use the temperature sensor to stir the mixture. 5. Once all of the ice is melted and the temperature reaches equilibrium, stop the program. Analyzing the Data: Part III - Heat of Fusion 1. Use the “zoom select” tool to zoom in on the region of the graph before mixing the water and ice. Record the temperature of the water before the mix in the data table. 2. Use the “zoom select” tool to determine the final temperature of the water after all of the ice has melted and it levels off. Record this in the data table as the final temperature. Part I - Specific Heat of Metal Data Table Metal Mass of empty Calorimeter Mass of Calorimeter + water Mass of water Mass of Metal Temperature of water before Temperature of metal before mix Final Temperature B 0.3746kg 0.5507kg 0.1761kg 0.0875kg 21.85 65.25 22.5 A 0.3726 0.4404kg 0.0658kg 0.842kg 22.91 68.3 25.1 Metal Specific Heat (J/goC) Lead 0.13 Copper 0.39 Stainless Steel 0.51 (approx.) Aluminum 0.91 1. Determine the specific heat of the metal in all trials. Compare it to the actual values by percent error. Part II: Heat Gain/Heat Loss Data Table Hot Water Cold Water Mass of empty cup 11.6g 11.1g Mass of cup + water 79.2g 76.8g Temperature before mix 40.45 22.25 Temperature after mix 31.2 31.2 Temperature change -9.25 8.95 1. Determine the Heat Gain 2. Determine the Heat Loss 3. Determine the percent difference between heat gain and loss (take the absolute value of heat loss). Part III - Heat of Fusion Data Table Mass of empty cup 11.1g Mass of cup and water 91.1g Mass of cup and water and ice 107.3g Mass of ice 16.2g Temperature of water before mix 41.25 Temperature of water after mix 20.1 Change in temperature of water -21.25 1. Determine the Heat Loss 2. Assuming that no heat is lost to the surroundings, calculate the heat of fusion. 3. Compare your heat of fusion of ice to the accepted value using percent error.

Explanation / Answer

specific heat of metal

heat lost by metal = heat gained by water

specific heat of metal = 0.1761 x 4.184 x (22.5 - 21.85)/0.0875 x (65.25 - 22.5)

                                   = 0.13 J/g.oC

The specific heat matches with that of Lead.

So metal is lead.

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