Expt08_Calorimetry
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Expt08_Calorimetry

Course Number: CHEM 16, Fall 2007

College/University: University of the...

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Date Performed: Experiment 8 Calorimetry I. Objectives: &gt; to determine the heat capacity of the calorimeter. &gt; to determine the enthalpy of reaction of <a href="/keyword/nitric-acid/" >nitric acid</a> and <a href="/keyword/sodium-hydroxide/" >sodium hydroxide</a> . II. Diagrams/Figures for Special Set-ups: III Outline/Schematic Diagram of Procedure.:...

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Date Performed: Experiment 8 Calorimetry I. Objectives: &gt; to determine the heat capacity of the calorimeter. &gt; to determine the enthalpy of reaction of <a href="/keyword/nitric-acid/" >nitric acid</a> and <a href="/keyword/sodium-hydroxide/" >sodium hydroxide</a> . II. Diagrams/Figures for Special Set-ups: III Outline/Schematic Diagram of Procedure.: &gt;Materials: Styrofoam cube or ball Thermometer 6&quot; test tube 50 mL graduated cylinder &gt;Procedure: Carve out a hole at a portion of the Styrofoam cube so that a 20 mL test tube could fit in completely and snugly. As shown on fig15, insert a 6&quot;test tube into this carved hole. Insert a thermometer into the rubber stopper such that the bulb of the thermometer would be positioned half way inside the test tube. Only the rubber stopper with the inserted thermometer would be visible on the surface of the Styrofoam cube. This is your improvised calorimeter. A. Calibration of the Calorimeter Pour 10.0 mL of 1.00 M HCl into the test tube of the constructed calorimeter. Record temperature vs. time data at 15-sec intervals until the temp reading is constant with time. This is your t initial. Remove the top of the calorimeter (w/c consists of the rubber stopper and the thermometer. Add 5.00 mL of 1.00 M NaOH. Immediately replace the top and record the temperature-time data at 30-sec intervals while swirling the contents occasionally. Continue taking temperature-time data until the temperature is constant or decreasing at a constant rate. This is your Tfinal. Make a graph of temp (in Celsius) vs time (in s). Compute for the heat capacity of the calorimeter, Ccal. Rubber stopper 1.00 M HCl 1.00 M NaOH 1.00 M HNO3 B. Determination of the Enthalpy of Reaction of <a href="/keyword/nitric-acid/" >nitric acid</a> and <a href="/keyword/sodium-hydroxide/" >sodium hydroxide</a> Measure 10.0 mL of 1.0 M HNO3 into the constructed calorimeter and determine tinitial similar to what was done in part A. Lift the top of the calorimeter and add 5.0 mL 1.0 M NaOH. Immediately replace the top of calorimeter and record temperature-time data at 15-sec intervals while swirling the contents occasionally. Continue taking temperature-time data until the temperature is constant or is increasing at a constant rate. This is your Tfinal. Make a graph of temp (in Celsius) vs. time (in sec). Compute for the enthalpy of reaction of <a href="/keyword/nitric-acid/" >nitric acid</a> and <a href="/keyword/sodium-hydroxide/" >sodium hydroxide</a> using the computed heat capacity of the calorimeter. IV. Special Notes: Waste Disposal: 1. Dilute all solutions with tap water and flush directly down the sink with copious running water. 2. Dispose the used Styrofoam into the Solid Waste container. V. Tabulation of Data:

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Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02
Logan University - CHEM - UG07120_02