X01-Smith-Joe

X01-Smith-Joe - Chm132L- X01-2004 1 Smith Joe Experiment 1:...

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Unformatted text preview: Chm132L- X01-2004 1 Smith Joe Experiment 1: Free Energy, Enthalpy, and Entropy I I.Purpose/Motivation : To measure the heat of neutralization for 2 weak acids by a strong base. II.Experimental Procedure : First, we determined the calorimeter constant for the calorimeter by measuring the temperature change two samples of water then their change after mixing. Then, we determined the heat of neutralization of acetic acid by sodium hydroxide by measuring the temperatures of the acid and base before mixing and every 20 seconds after until the temperature stopped changing. We repeated this step to verify the data then repeated it with chloro-acetic acid and sodium hydroxide twice following the same procedure as with acetic acid. III.Data: Data Set for Water for Determination of the Calorimeter Constant Time Temp of Hot Water (°C) Temp of Cold Water (°C) Temp of Mixture (°C) 29 21.5 24.2 20 30.2 21.5 25.4 40 30.1 21.5 25.5 60 30.2 21.5 25.6 80 30.1 21.5 25.6 100 30 21.5 25.6 120 30 21.5 25.6 140 30 21.4 25.6 160 29.9 21.4 25.6 180 29.9 21.4 25.6 200 29.9 21.4 25.6 220 29.8 21.4 25.6 240 29.8 21.4 25.6 Chm132L- X01-2004 2 Smith Joe The initial temperature for the acetic acid was 22.7°C for the first and second trials, and, for the sodium hydroxide, the temperatures were 22.8°C and 22.6°C for the first and second trials respectively. Heat Over Time of Reaction Between Acetic Acid with Sodium Hydroxide Time Temp of Mixture (°C) Trial 1 Time 2 Temp of Mixture (°C) Trial 2 25.2 23.4 10 26.8 10 27.3 20 29.5 20 28.8 30 29.7 30 29.3 40 29.8 40 29.4 50 29.8 50 29.5 60 29.8 60 29.6 80 29.8 70 29.6 100 29.8 80 29.6 120 29.8 90 29.6 100 29.6 120...
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This note was uploaded on 04/20/2008 for the course CHM 132 taught by Professor Farrar during the Spring '08 term at Rochester.

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X01-Smith-Joe - Chm132L- X01-2004 1 Smith Joe Experiment 1:...

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