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Material Type: Lab; Class: General Physics-GTSC1; Subject: Physics; University: Mesa State College; Term: Fall 2007;
Typology: Lab Reports
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Phys 111L Fall 2007
When heat is added to or removed from an object at constant volume or pressure, a change in temperature results. The relationship between the magnitude of the heat Q and the corresponding change in temperature depends on the object and is given by
Q = mc∆T (1)
where m is the mass of the object and c its specific heat. In this experiment, you will investigate this relationship for various materials.
1 Experiment: Water at different temperatures In this part of the experiment, you will mix two cups of water initially at different temperatures and determine the heat which is transferred.
a) Start DataStudio and connect the temperature sensor. Display the temperature in a graph and a digits windows. b) Fill one cup less than halfway with water at room temperature. Determine the mass of the water in the cup. c) Fill another cup less than halfway with hot water. It will be important that the water from both cups can be entirely accommodated in just one of the cups. Determine the mass of the water in the cup. d) Measure the temperature of the water in each cup. Ensure that the thermometer does not touch the sides of the cup and stir the water while you measure. e) Pour all of the water from one cup into the other and observe the temperature. Measure the equilibrium temperature of the mixed water. f) Determine the heat lost by the warmer water. g) Determine the heat gained by the cooler water. h) Determine the percentage difference between the heat lost by the warmer water and that gained by the cooler water.
2 Experiment: Specific heats of metals In this experiment you will determine the specific heats of aluminum and copper. The metal can be heated by immersing it in hot water, waiting for it to reach equilibrium and then measuring the water temperature. Subsequently the metal can be immersed in cool water, allowing for a heat transfer from the metal to the water.
a) Determine the mass of the aluminum.
b) Fill the polystyrene cup with just enough water to submerge the metal. Determine the mass of the water and allow it to reach room temperature. Measure and record the temperature. c) Pour enough hot water to cover the metal into a beaker. While recording the temperature, immerse the metal in the hot water. When it reaches equilibrium, record the temperature of the metal. d) Quickly remove the metal from the hot water and place it in the cool water. Observe the temperature and wait until it reaches equilibrium and then record it. e) Determine the heat gained by the aluminum and use this to determine the specific heat of aluminum. f) Repeat the entire procedure for copper.
3 Homework
a) One mole of copper has mass 63.55 g. The specific heat capacity of copper is 386 J/kg·K. Determine the heat capacity of one mole of copper per in J/K. b) One mole of aluminum has mass 26.98 g. The specific heat capacity of copper is 897 J/kg·K. Determine the heat capacity of one mole of copper per in J/K. c) Suppose that in the experiment involving aluminum, the thermometer was only accurate to 1◦^ C. By how much would this affect the calculated specific heat of the aluminum? As an example, consider 50 g of aluminum initially at temperature 80 ◦^ C placed into 100 g of water initially at temperature 20◦^ C. The final tempera- ture of the water and aluminum is measured (with the imprecise thermometer) to be 26◦^ C. Determine the specific heat of the aluminum using this. However, the im- precision of the thermometer is such that one could reasonably conclude that the final temperature was 25◦^ C. Determine the specific heat of the aluminum using this. Determine the percentage difference between the two values for the specific heat of aluminum.