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

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
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
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

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).

Page1 / 2

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

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online