lab 4.docx - Experiment#4 Calorimetry of Reactions of...

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Experiment #4 Calorimetry of Reactions of Magnesium and Magnesium Oxide Mary Frances Johnson Vikram Balaji 20 February, 2018 CHEM 1310 Section C27 TA: Shaoren Yuan Honor Pledge – Freshman Chemistry Laboratories I did not copy any portion of this work from the work of other students, old lab reports, or unreferenced materials. I understand that such activity is a violation of the Georgia Tech Honor Code. ______________________________________ Signature
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Data and Results: Table 1. Data for Calibration of Calorimeter Trial Cold T (ºC) Hot T (ºC) Final T (ºC) C cal (J/ºC) 1 20.4 54.8 36.9 10.65 2 22.5 50.9 36.1 11.07 Mean C cal 10.87 St. Dev. 0.215 Table 2. Calorimetry of Mg + HCl Trial Initial T (ºC) Final T (ºC) Mass Mg (g) Volume HCl( aq ) (mL) H (kJ/mol) 1 20.8 27.3 0.085 60.0 -486 2 20.1 26.9 0.088 59.7 -492 Mean -489 St. Dev. 2.5 Table 3. Calorimetry of MgO + HCl Trial Initial T (ºC) Final T (ºC) Mass MgO (g) Volume HCl( aq ) (mL) H (kJ/mol) 1 20.0 24.8 0.417 59.9 -122 2 19.9 25.2 0.416 59.1 -134 Mean -128
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St. Dev. 6.11 Discussion: The goal of part A of the experiment was to determine the heat capacity of the calorimeters that were to be used for parts B and C of the experiment. To do this, the heat capacity of the calorimeter was found experimentally in two trials. The mean heat capacity was found to be 10.87 J/ºC with a standard deviation of 0.215 J/ºC. In the first trial, the heat capacity of the calorimeter was calculated by setting the heat lost by the hot water equal to the sum of the heat gained by the cold water and the heat absorbed by the calorimeter. The heat values used derived from the equation q = mC ∆T , where q is the heat released or absorbed in Joules. Using the following calculations, the heat capacity of the calorimeter was found.
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