exp 1 - hot and coldpacks - Results and Discussion: The...

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Results and Discussion: The heat capacity of a calorimeter and the heats of solution of several ionic salts were determined by using constant-pressure calorimetry. The heat capacity was determined by using the equation: -C∆T = ms∆ Thot + ms∆ Tcold and the heat of solution for a salt was determined by using the equation: -∆Hsoln = C cal · ∆T cal + m mix · S mix · ∆T mix. Week 1: Determination of the Heat Capacity of the Calorimeter A calorimeter was assembled with distilled water and the temperature change of both the cold and hot water were recorded. The hot water was placed into the calorimeter with cold water and the equilibrium temperature was found. Trial Mass Hot H2O (g) Mass Cold H2O (g) ∆T hot (°C) ∆T cold (°C) Heat capacity (J/°C) 1 44.125 46.462 -3.4 3.1 8.080 2 43.873 49.099 -5.4 4.5 14.833 3 51.847 47.171 -3.9 4.8 -21.089 4 49.12 45.707 -4.3 3.6 54.190 1 The change in temperature of the cold water is the same as the change in temperature of the calorimeter. The data was then plugged into the first equation stated above and the heat capacities for each trial were determined.
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This note was uploaded on 02/28/2008 for the course CHEM 342132 taught by Professor Davis during the Spring '08 term at Cornell University (Engineering School).

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exp 1 - hot and coldpacks - Results and Discussion: The...

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