An experiment of the soda can to perform the calorimetry, Lab Reports of Chemistry

Download An experiment of the soda can to perform the calorimetry and more Lab Reports Chemistry in PDF only on Docsity! Name Period Soda Can Calorimeter In this experiment, the specific heat of water and its change in temperature will be used to determine the caloric content of a food sample. The normal unit for measuring the energy content in food is called a Calorie (with an uppercase C). A Calorie is really a kilocalorie, or 1000 calories (lowercase c). During calorimetry, food burns and its stored energy is quickly converted into heat energy and products of combustion (carbon dioxide and water). The heat energy that is released is then transferred into the water above it in the calorimeter. The temperature change in the water is then measured and used to calculate the amount of heat energy released from the burning food. The heat energy is calculated using Q = mCp∆T. 1 calorie (cal) = 4.18 joules (J) 1000 calories (cal) = 1 Calorie (Cal) = 1 kilocalorie (kcal) Procedure 1. Place a food sample on the food holder. Measure and record the combined mass of the food holder and sample. 2. Using a graduated cylinder, measure and add 50.0 mL of water to an empty, clean soda can. Record the amount of water you put into the can as grams (1mL = 1 g). 3. Bend the tab on the soda can and slide a stirring stick through the hole. Suspend the can on a support stand using a metal ring. Adjust the height of the can so you can hold the food under it. 4. Insert a thermometer into the can. Measure and record the initial temperature of the water. 5. Light the food sample and center it under the soda can. Allow the water to be heated until the food sample stops burning. Record the maximum (final) temperature of the water in the can. 6. Measure and record the final mass of the food holder and sample. 7. Clean the bottom of the can and remove any food residue from the food holder. 8. Repeat steps 1–7 two more times with two different snack food samples. Pre – Lab 1. What is the First Law of Thermodynamics? 2. How are the particles in a hot object different from the particles in a colder object? 3. Explain how the heat gets transferred. 4. Why would it be important to make sure the flame is touching the can? 5. How many calories are in 1 Calorie (nutritional calorie)? 6. How many calories are in 1 Joule? 7. Convert the following values. a. 500 calories = _________________ Calories b. 435 calories = _________________ Joules c. 0.23 Calories = _________________ Joules d. 5671 Joules = _________________ Calories 8. Fill out the following table (you will need this for post lab questions) Food Item Calorie Content (Calories per serving) Serving Size (grams) Fuel Value (Calories per gram) Heat Value (Joules per gram) Cashews 238 50 Hot Cheetos 160 28 Marshmallow 90 26 9. The burning of a 0.37 g potato chip cause the temperature of 58.18 g of water in a soda can calorimeter to increase from 21.5oC to 28.1oC. Calculate the amount of heat absorbed by the water. The specific heat of water is 4.18 J/goC. 10. Convert the above answer to Calories.