Specific Heat of Solids and Liquids Part II

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1 Specific Heat of Solids and Liquids Part II From your previous experiments with rocks and water you have determined that the specific heat of a rock is less than that of water. What about other substances? Are there substances that have a higher specific heat than water? As it turns out, water has one of the highest specific heats of any substance. In other words, it takes a lot of heat to raise the temperature of water. (In other words, it takes a long time for a pot of water to boil or to cool down. This is just one of the many unusual properties of water. In this next experiment, you will compare the specific heat of the rock to that of lead and aluminum. First, make a hypothesis. Compared to the rock, do think lead has a higher or lower specific heat? Explain. Compared to the rock, do think aluminum has a higher or lower specific heat? Explain. We have available several samples of aluminum and lead. Your job is to carry out an experiment to measure the specific heat of these metals. You can use a procedure similar to the one used with the rocks. It will not, however, be necessary for the mass of the metal to equal the mass of the water. What is the minimum amount of water you need to cover the metal you are using? (Write the number below for lead and aluminum).

2 In the space below, describe the experimental procedure that you will use to find the specific heat of each metal. Be specific and clear. Use the tables listed below to record the results of your experiment: Aluminum Mass of Aluminum (g) Mass of Water (g) Trial 1 Trial 2 Trial 3 of Aluminum ( o C) Final Temperature Lead Mass of Lead (g) Trial 1 Trial 2 Trial 3 Mass of Water (g) of Lead ( o C) Final Temperature

3 Use your data to calculate the specific heat of each metal. If you ve forgotten how to do this, look back your experiment with the rock and water and use the same method. Show your work in the space below (include units!). Check your results with an instructor when you re finished. Calculated Specific Heat of Aluminum: Calculated Specific Heat of Lead: Compare your results with your initial hypothesis. Were the results consistent with what you expected? Why or why not?

4 END OF MODULE QUESTIONS: Specific Heat Answer the following questions on another sheet of paper. 1. A cup with 40 grams of 90 C water is mixed with a cup with 70 grams of water at 10 C. a. Predict the final temperature of the water. Explain your reasoning. b. Calculate the expected final temperature of the water. (Assume that no heat is lost to the surroundings) calories of heat were added to both a sample of water and a sample of copper. a) The 10 calories of heat increased the temperature of a sample of water by 5 C. What was the mass of the water? b) The 10 calories of heat increased the temperature of 22 g of copper by 5 C. Find the specific heat of copper. 3. In a lab experiment, an 80 g sample of water at 20 o C is mixed with 80 g of aluminum at 50 o C. The specific heat of aluminum is 0.20 cal/g o C. In other words, it takes only 0.2 calories to raise the temperature of 1 g of aluminum by 1 o C. a. What is your estimation of what the final temperature of the mixture will be? (Do not do any calculations yet). Explain your reasoning. b. How many calories are required to change the temperature of 1 gram of aluminum by 5 o C? Show your work. c. How many calories are required to change the temperature of 80 grams of aluminum by 5 o C? Show your work. d. Complete the following table by filling in the number of calories needed to change the temperature of the aluminum by 5 o C, and the resulting temperature change of the cold water. Continue until you have determined the final temperature of the mixture. (Note: if you have trouble doing this in 5 o C increments, you can do it in 1 o C increments, but it will take many more steps) Total Calories Transferred Temperature of 80 g of aluminum 0 50 o C 45 o C Temperature of 80 g of cold water 20 o C

5 e. What is the final temperature of the mixture? f. How many total calories are transferred? g. What is the temperature change of the water in this experiment? h. What is the temperature change of the metal in this experiment? g. Compare the heat lost by the metal to the heat gained by the water. Explain your reasoning. 4. a. How would your results have differed in the experiment you conducted in Part 2 (with metal and water) if you had used ½ as much water. b. How would your results have differed if you had used twice the amount of water in this experiment?

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