Lab Report 4 - John Xu Experiment 4 Enthalpy of Formation of an Ammonium Salt Part I Determination of the Heat Capacity of the Calorimeter Mass of

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John Xu 3/8/07 Experiment 4: Enthalpy of Formation of an Ammonium Salt Part I: Determination of the Heat Capacity of the Calorimeter Mass of Cold Water: 48.0 grams Mass of Hot Water: 44.4 grams Initial Temperature of Cold Water: 22.7 °C (y = -0.0007(70 sec) + 22.75) Initial Temperature of Hot Water: 42.9 °C (y = -0.0173(70 sec) + 44.15) Final Temperature of Mixture: 30.6 °C (y = -0.0032(70 sec) + 30.864) ∆T cold : 7.9 °C ∆T hot : -12.3 °C ∆T calorimeter : 7.9 °C C calorimeter = [(-44.4 g)(4.184 J/g • °C)(-12.3 °C)-(48.0 g)(4.184 J/g • °C)(7.9 °C)]/(7.9 °C) = 88 J/ °C Part II: Neutralization Trial 1: Mass of Solution: 72.5 g Initial Temperature of NH 3 : 20.7 °C Final Temperature of Solution: 35.0 °C (y = -0.0019(70 sec) + 35.119) ∆T soln : 14.3 °C ∆T calorimeter : 14.3 °C -q neutralization = (72.5 g)(4.184 J/g • °C)(14.3 °C)+(88 J/ °C)(14.3 °C) = 5600 J n Limiting : 0.0375 moles ∆H neutralization : -5600 J/ 0.0375 mole= -150 kJ/mol Trial 2 Mass of Solution: 75.1 g

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This note was uploaded on 04/07/2008 for the course CHEM 211 taught by Professor Crane, b during the Spring '06 term at Cornell University (Engineering School).

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Lab Report 4 - John Xu Experiment 4 Enthalpy of Formation of an Ammonium Salt Part I Determination of the Heat Capacity of the Calorimeter Mass of

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