Chem Exp. Rep. 4

Chem Exp. Rep. 4 - 03/09/08 Experiment Report: Enthalpy of...

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03/09/08 Experiment Report: Enthalpy of Formation of Ammonium Salts PURPOSE: The purpose of this experiment was to calculate the enthalpy of several reactions, including the enthalpy of neutralization of Hydrochloric Acid with Ammonia, the calorimeter constant, and the enthalpy of dissolution of Ammonium Chloride. To calculate the enthalpies of each of these reactions, we first had to measure the temperature change before and after the mixing of the solutions and then extrapolate the temperature change from the graph. After extrapolating this temperature changes in each of the reactions, you can then use the enthalpy of neutralization and the enthalpy of dissolution to calculate the enthalpy of formation of Ammonium Chloride. RESULTS AND DATA: Trial #1: [HCl]= 2.00M [NaOH]=2.05M Time, min Temp HCl 0 22.9 .5 22.9 1.0 23.0 1.5 23.0 2.0 23.0 2.5 23.0 3.0 23.0 3.5 23.0 4.0 23.0 4.5 23.0 After Mixing: 23.0 C Time, min. Temp. Time, min Temp. NaOH 0 22.8 .5 22.9 1.0 23.0 1.5 23.0 2.0 23.0 2.5 23.0 3.0 23.0 3.5 23.0 4.0 23.0 4.5 23.0
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6.0 36.5 7.0 36.5 8.0 35.5 9.0 35.5 10 35.2 11 34.7 12 34.7 13 34.5 14 34.2 Trial #2: Time, min Temp. NaOH Temp HCl 0 23.4 23.5 0.5 23.4 23.5 1.0 23.4 23.5 1.5 23.5 23.5 2.0 23.5 23.5 2.5 23.5 23.5 3.0 23.5 23.5 3.5 23.5 23.5 4.0 23.5 23.5
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Chem Exp. Rep. 4 - 03/09/08 Experiment Report: Enthalpy of...

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