Instructions: Complete each section of this report and answer all questions in complete sentences for full credit. Materials: thermometer, two foam cups, measuring cup from your kitchen, hot water, and one liquid selected from the chart below and placed in your refrigerator for one or more hours before you begin your activity Liquid Heat capacity (J/(g oC)) Density (g/mL) Grape juice 3 1. Whole milk 3 1. Orange juice 3 1. Tomato juice 3 1. Caution: You will be working with hot water in this lab. Be very careful as you pour so you do not burn yourself. Also, be sure to read your thermometer carefully. The numbers on the thermometer scale refer to the line under the number. Lastly, it's important to perform certain steps quickly and efficiently to minimize heat loss to the surroundings. Procedure: 1. Read the entire procedure before you begin the experiment. 2. Use the metric scale on your measuring cup to measure 237 mL (1 cup) of your selected refrigerated liquid. Pour this liquid into one of the foam cups. 3. Now, get the hottest water possible from the faucet on your sink. Use the metric scale on your measuring cup to measure 237 mL (1 cup) of hot water. Pour this water into the other foam cup. 4. Quickly measure the temperature of the cold liquid and the hot water. Record the temperatures in a data table. 5. Very quickly pour the hot water into the cold liquid. Place the thermometer in the mixture. Invert the cup that contained the cold liquid over the cup containing the water mixture. 6. Keeping the bulb of the thermometer in the liquid, check the temperature reading about every 20 seconds until the temperature stabilizes. Keep the lid (inverted cup) in place as much as possible. When the temperature is constant (this will happen very quickly), record this temperature in a data table as the final temperature. Unless Otherwise Noted All Content © 2022 Florida Virtual School. FlexPoint Education Cloud™ is a
Data Create a data table of for your measurements and calculations. Two measurements are provided for you. Record the other measurements needed for this activity. Measurement Type Measurement Value Volume of cold liquid 237 mL (1 cup) Volume of hot water 237 mL (1 cup) Beginning temperature of the cold liquid (oC) 10 oC Beginning temperature of the hot water (oC) 46 oC Final temperature of the cold liquid/hot water mixture (oC) 27 oC Change in temperature of the cold liquid (oC) 17 oC Change in temperature of the hot water (oC) -19 oC Mass of the cold liquid (g) 249 g Mass of the hot water (g) Calculations 1. Record the calculations below in your data table. A. Use the beginning temperature of the hot water and cold liquid and the final temperature (Tf) of the mixture to calculate the change in temperatures of the cold liquid and the change in temperature of the hot water. B. Since one milliliter (mL) of water has a mass of one gram, it is very easy to determine the mass of the cold liquid and hot water. For example, if you have 100 mL of water, then the mass of the water is 100 g. Unless Otherwise Noted All Content © 2022 Florida Virtual School. FlexPoint Education Cloud™ is a
Conclusion 1. Compare the values for heat gain and heat loss in calculations 2 and 3. Were they the same value? What might have caused the difference in values? The calculations in 2 and 3 were not the same value. One cause that there were a difference in the values could have been because of the different methods or different formulas that could be a factor in why there was a difference in values. 2. In a closed system, the total heat given off by warmer substances equals the total heat energy gained by cooler substances. Which process in your activity was endothermic? Which process was exothermic? The process in which energy or heat was gained in my liquid was endothermic. The lose of energy or heat was exothermic which in occurred from the water. 3. Create a diagram to illustrate and describe the movement of heat between both liquids in the calorimeter. Be sure to label all heat transfers between liquids, including any heat lost to the surroundings. 4. How did this activity demonstrate conservation of energy? This activity demonstrates conservation of energy because the conservation of energy states that in a closed system, the energy of interaction objects or particles remain constant. It also states energy is neither created nor destroy. This activity shows how energy is gained or lost from the water equal to how much was lost and water in OJ.
represent an increase or decrease in entropy? Explain your answer. This mixing of two substances would increase the entropy because there would be a greater volume for particles to distribute throughout. Unless Otherwise Noted All Content © 2022 Florida Virtual School. FlexPoint Education Cloud™ is a
