c) What is the relationship between the heat gained/lost by the metal and the heat gained/lost by the water?
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1 Chem 1314 Web Laboratory Fall 2013 Name TA Name Lab Section # Pre-Laboratory Questions: 1. In this experiment you will be immersing a piece of metal that has been heated to a known temperature into a sample of water of known temperature (room temperature). ly the temperature of the metal is higher than the temperature of the water. a) When a piece of hot metal is added to the water (initially at a temperature around room temperature) does the metal gain or lose heat? Explain. b) When a piece of hot metal is added to the water (initially at a temperature around room temperature) does the water gain or lose heat? Explain. c) What is the relationship between the heat gained/lost by the metal and the heat gained/lost by the water? d) After adding the piece of metal to the water, how are the final temperature of the metal and water related? CHEM FALL 2013
2 The goal of this experiment is to investigate what happens when a piece of hot metal is added to a sample of water at or near room temperature. NOTE: I expect each student to collect their own, unique set of data for the experiments in this activity. Activity 1. Comparison of the heat exchanged by metals Start the simulation ( hem/heat_metal.html). In the upper left corner of the simulation is a list of six metals, four with names and two unknown metals. For the experiment select two metals to work with according to the table below; OSU Student Number (last digit) #1 #2 0 or 1 Silver Copper 2 or 3 Gold Iron 4 or 5 Silver Iron 6 or 7 Copper Gold 8 or 9 Iron Copper ACTIVITY #1: Make a prediction of which of your two metals, initially at a high temperature, will raise the temperature of a sample of water the highest. You need to make a fair comparison. For example if when you test the metals they should have the same mass and the same initial temperature, and be added to a sample of water of the same mass and the same initial temperature. The initial temperature of the metal (T i ) should be greater than the initial temperature of the water (T i ' ). Complete the following: 1a. Identify your #1: Identify your #2: 1b. Prediction (which metal will raise the temperature of the water the highest?): # : 1c. Explain how you arrived at your answer. CHEM FALL 2013
3 2. Use the computer simulation to do your experiment. Record your data below. The J specific heat of water is 4.18 g C. The density of water is 1.00 g/ml. DATA: (Enter the name of one of your metals, and record the initial mass and temperature for both the metal and for water. Click on the Start button and observe what happens. Record the final temperature for the metal and for water. Repeat this in the second table for the other metal assigned to you.) Experiment #1 (#1) Experiment #2 (#2) Did your prediction (1b) match your experimental results? Explain. In the two experiments above, heat was transferred from to CHEM FALL 2013
4 Repeat the experiments you just performed with a different mass of the metal, a different initial temperature of the metal, a different mass of the water and but the same initial temperature of the water. Record your observations below. Experiment #3 (#1) Experiment #4 (#2) In the two experiments above, heat was transferred from to CHEM FALL 2013
5 CALCULATIONS: 3a. For each experiment (Part 2) calculate the heat that was exchanged (absorbed or released) by the water. You may use the formula q = mc T. Show all steps and be sure to include units in all steps and in your answer. Be sure to indicate the "sign" (i.e. positive or negative). Experiment #1 Experiment #2 3b. For each experiment (in Part 2) calculate the heat that was exchanged (absorbed or released) by the metal. Show all steps and be sure to include units in all steps and in your answer. Be sure to indicate the "sign" (i.e. positive or negative). Experiment #1 Experiment #2 3c. Compare the values of the heat exchanged by the water and the metal. Within experimental error, was the Law of Conservation of Energy obeyed? Experiment #1 Experiment #2 CHEM FALL 2013
6 3a. For each experiment (Part 2) calculate the heat that was exchanged (absorbed or released) by the water. You may use the formula q = mc T. Show all steps and be sure to include units in all steps and in your answer. Be sure to indicate the "sign" (i.e. positive or negative). Experiment #3 Experiment #4 3b. For each experiment (in Part 2) calculate the heat that was exchanged (absorbed or released) by the metal. Show all steps and be sure to include units in all steps and in your answer. Be sure to indicate the "sign" (i.e. positive or negative). Experiment #3 Experiment #4 3c. Compare the values of the heat exchanged by the water and the metal. Within experimental error, was the Law of Conservation of Energy obeyed? Experiment #3 Experiment #4 CHEM FALL 2013
7 ACTIVITY #2: 4a. If you double the mass of #1 in Part 2 Experiment#1, keeping everything else the same, predict what will happen to the T of the water? 4b. If you double the mass of water in Part 2 Experiment#1, keeping everything else the same, predict what will happen to the T of the water? Do these two experiments using the computer simulation. DATA: Experiment #1 (#1) Experiment #2 (#2) Did your predictions (in Part 4) match the results of the computer simulation? Explain. CHEM FALL 2013
8 ACTIVITY #3: Determination of the specific heat of an unknown metal. 5. Select one of the unknown metals ( X or Y) to work with according to the table below; OSU Student Number (last digit) Unknown 0-4 X 5-9 Y Your is, Design and carry out an experiment that will help you determine the specific heat of this metal. Write the experimental procedure you used to determine the specific heat of the unknown metal. (NOTE: Your procedure must be detailed enough that another student unfamiliar with this experiment would be able to reproduce the data you obtain. What observations did you collect?: (You may or may not need all of the cells below.) CHEM FALL 2013
9 Using your observations indicate the Evidence you have to support the Claim you will make below. Claim: The specific heat of metal is. CHEM FALL 2013
10 POST-LAB Questions: 1a. A piece of metal at a high temperature was added to g of water initially at C. When the temperature of the water with the piece of metal was measured again the final temperature was C. Calculate the amount of heat absorbed by the water. b. How much heat did the metal give off in this experiment? c. If the mass of the metal was 70.0 g and the initial temperature of the hot metal was C, calculate the specific heat of the metal. 2. A piece of silver weighing grams is heated to C and added to g of water initially at C. Calculate the final temperature of the mixture. 3. A sample of metal weighing 95.0 g is heated to C and added to 115 g of water initially at C. The final temperature of the mixture is C. Identify the metal as silver, gold, copper, or iron. CHEM FALL 2013
OSU Student Number (last digit) Metal #1 Metal #2 0-1 Silver Copper 2-3 Gold Iron 4-5 Silver Iron 6-7 Copper Gold 8-9 Iron Copper
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