Part D: Enthalpy change for the neutralization reaction of CH3COOH(aq) and NaOH (aq) 1. Mass of CH3COOH solution .g 2. Initial Temperature of CH3COOH solution in calorimeter °C 3. Mass of NaOH solution 4. Final temperature of the solution °C 5. Mass of the final solution (NaOH + CH3COOH) 7. Change in temperature, AT °C 8. Was the reaction endothermic or exothermic? 9. Heat absorbed/released in joules by solution Can = meol X CsX AT (Cs = 4.184 J/g°C) 10. Heat absorbed/released by reaction in kilojoules kJ Csol + ann =0 11. Moles of CH3COOH mol Assume density of CH3COOH solution d = 1.0 g/mL Molarity = 1.0 M 12. Change in enthalpy for the reaction of CH3COOH+ NAOH kJ/mol AH=9
Part D: Enthalpy change for the neutralization reaction of CH3COOH(aq) and NaOH (aq) 1. Mass of CH3COOH solution .g 2. Initial Temperature of CH3COOH solution in calorimeter °C 3. Mass of NaOH solution 4. Final temperature of the solution °C 5. Mass of the final solution (NaOH + CH3COOH) 7. Change in temperature, AT °C 8. Was the reaction endothermic or exothermic? 9. Heat absorbed/released in joules by solution Can = meol X CsX AT (Cs = 4.184 J/g°C) 10. Heat absorbed/released by reaction in kilojoules kJ Csol + ann =0 11. Moles of CH3COOH mol Assume density of CH3COOH solution d = 1.0 g/mL Molarity = 1.0 M 12. Change in enthalpy for the reaction of CH3COOH+ NAOH kJ/mol AH=9
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...
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Neutralize of acetic acid and sodium hydroxide
50ml of CH3COOH set at 1 M
50ml of NaOH set at 1 M
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