Chem 111Stephen Fike

Chem 111Stephen Fike - Chem 111 10 / 16 / 07 Stephen Fike...

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Chem 111 Stephen Fike 10 / 16 / 07 Chris Coble 10 / 30 / 07 Objective: The objective of this experiment was to determine heats of neutralization and solution by using a simple calorimeter. By using data constructed through the use of the calorimeter in conjunction with computed data from Hess’s law, we were able to compute the heat of formation of a chemical compound NH 4 Cl. Data Table: Enthalpy Reaction of NH 3 + HCl NH 4 Cl Trial 1 Trial 2 Time (min) Temperature ( o C) Temperature ( o C) 0 23 19.9 .5 21.5 20.83 1 21.3 21.0 1.5 21.2 21.05 2 21.1 21.06 2.5 21.1 21.07 3 21.08 21.09 3.5 Add HCl Add HCl 4 30.4 30.9 4.5 30.63 30.6 5 30.65 30.68 5.5 30.58 30.62 6 30.5 30.6 6.5 30.5 30.55 7 30.48 30.5
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7.5 30.39 30.45 8 30.36 30.4 8.5 30.3 30.3 9 30.25 30.28 9.5 30.19 30.2 10 30.18 30.17 10.5 30.1 30.1 11 30.07 30.09 NH 4 Cl (s) NH 4 Cl (aq) Trial 1 (4.0929g) Trial 2 (4.0764g) Time (min) Temperature o C Temperature o C 0 20.15 20.18 .5 20.12 20.09 1 20.11 20.09 1.5 20.11 20.09 2 20.1 20.09 2.5 20.1 20.09 3 20.1 20.09 3.5 Add NH 4 Cl Add NH 4 Cl 4 18.45 18.4
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4.5
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Chem 111Stephen Fike - Chem 111 10 / 16 / 07 Stephen Fike...

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