Dolores RamirezExperiment #9-Charles’s Law: Determination of Absolute ZeroDolores RamirezChem 2 Lab 2LoganApril 21, 2013Experiment #9-Charles’s Law: Determination of AbsoluteZero1. Introduction: The purpose of this lab is to explore the relationship between the temperature and volume of a gas. We will also evaluate the temperature at which the volume of an “ideal” gas extrapolates to a minimum value (zero).2. Experimental:a) Materials:None.b) Apparatus:125-mL Erlenmeyer flask with fitted 1-hole stopper and glass tube; flask clamp; wax pencil; 600-mL beaker and hot plate.c) Procedure: 1. Get a rubber stopper with a glass tube in it and insert it into a 125 mL Erlenmeyer flask. Flask must me dry. Then mark the lower level of thestopper with a wax pencil.2. Place a 600 mL beaker on a hot plate and use an adjustable clamp to clamp the flask so that as much of it as possible is below the rim of thebeaker, without touching the bottom. Add water to the 600 mL beaker to cover as much of the flask as possible. Do not overfill.3. Heat water till eater boils and continue heating for about 10 minutes. At this point you may assume that the air in the flask is now the same temperature as the water. Record the temperature of the boiling water. May be slightly below boiling point.4. Prepare room temperature water bath by filling pan with room temperature water. The pan should be 3.4 filled.5. Place your finger over the end of the tube and, using the clamp as a handle, remove the flask from the boiling water bath. Invert the flask in a water bath at a low temperature and remove your finger from the tube after the flask is submerged. Swirl the flask around in the pan to allow the water temperature to equilibrate. Keep the flask submerged for at least five minutes. Record the temperatures of the water used to cool flask.6. Equalize the pressure within the flask with the atmospheric pressure byraising the flask until the water level inside and outside the flask are the same. While the end of the tube is still submerged, place your 1finger over the end of the tube, remove the flask from the water and setit upright on the bench top. Remove the stopper assembly and, using your graduated cylinder, fully measure the volume of water in flask. Record this as the volume change upon cooling the lower temperature. Now fill the flask with water up to the wax line on the flask. Measure this volume and record as the original volume of the hot air.7. Empty the flask into the sink and dry it thoroughly. Repeat the entire procedure, but this time, invert the flask in a pan of water at a differenttemperature, ice cold water. Again, be sure to eliminate any temperature gradients by stirring while the flask is cooling. Record the temperature of the water and the volume change upon cooling. Pour the water in the pan and in the flask down the sink when you are done.8. Record the barometric pressure in the laboratory. Because you have equalized the water levels inside and outside the flask, this is equal to the pressure of the air in the flask. You will need this value in your calculations. Record the % relative humidity. 3. Results and Discussion:All results to this experiment are found on page 4. We were able calculate all data points to this experiment. The data point for the air in boiling bath water was at 100 degrees Celsius and the volume was at 144.58mL. The data point for atroom temperature was 22 degrees Celsius which is little below room temperature and the volume was at 114.90mL. The air for the ice-cold bath water was 0 degrees Celsius and the volume was at 101.37mL. The equation that I came up with do to these data points was y = 0.4185x + 103.26R^2 = 0.99.Do to this equation we were able to calculate the % relative error which came out to be 9.67 relative error%.4. Conclusion:As conclusion this experiment was successful. We were able to successfully explore the relationship between the temperature and volume of a gas. We were also evaluate the temperature at which the volume of an “ideal” gas extrapolates to a minimum value (zero). We were able to calculate all data points for hot, room temperature, and ice cold water. The data that was calculated help in plotting the temperatures into a graph that calculated are equation which then help us calculate the% relative error. Based on my experimental results, my points and graph show that as temperature increases, volume also increases, which supports Charles’ Law.a) Initialed Duplicate Laboratory Notebook Page(s):i. The initialed duplicate laboratory notebook page(s) must be included after your conclusion upon report submission.25. Report Questions:1)2) Equation of line using Excel: y=volume (mL); x=temperature (°C)When v=0 = y=00 = 0.4185x + 103.26-103.26 = 0.4185xx = -246.74Temp. = -246.74°C%relative error=experiment value−accepted valueaccepted value×100 %¿−246.74−(−273.15)273.15×100 %=9.67 %3) Based on my experimental results, my points and graph show that as temperature increases, volume also increases, which supports Charles’ Law (increasing temperature is directly proportional to volume). My value for absolute zero was -246.74°C and my relative error was 9.67%. Possible errors could be timing the experiment, having little/ too much ice in ice bath, room temperature water sitting outfor too long. Methods to minimize the error would be to improve timing in experiment, constantly keep an eye on the experiment, leave thermometer in boiling water for sufficient time, have a good amount of ice for bath, and don’t let room temperature water to sit for too long.4)a. If some water was in the flask, then the calculations would yield inaccurate volume. b. You would equalize the water level in the Erlenmeyer flask and the pan of water so the pressure in the flask (water and air) is equal to the pressure of the surrounding atmosphere,3y = 0.4185x + 103.26R^2 = 0.99c. Since temperature and volume are directly proportional with one another, thentemperatures below -273 Celsius would yield a negative volume, which is not possible. It’s not possible because volume of a gas cannot be negative, because gas particles must occupy space, meaning the volume cannot be