Experiment 11

Experiment 11 - Experiment 11: Calorimetry and Hesss Law...

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Experiment 11: Calorimetry and Hess’s Law Kim Smith Chemistry 122 1/14/11 T.A.- Antony Akura Okumu
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Purpose: To be able to determine change in enthalpy for four reactions using calorimetry and Hess’s Law. Procedure: Refer to pages 6-7 of Laboratory Experiments in General chemistry, Volume 2 by Judith Casey and Robert Tatz, Hayden McNeil Publishing, Winter 2011- Spring 2011. Report Sheet: See attached report sheet Sample Calculations: Sample Calculations Part A 9 and 10: 9. Heat gained by water q water = Mass of H 2 O x 4.18/g© x Δ T q water = 59.22g x 4.18/g© x 7.5 © = 1.9 x 10 3 J 10. Heat capacity of calorimeter (C) q calorimeter = C x (T f – T i ) © -q cu = q water + q calorimeter q calorimeter = -q cu - q water q calorimeter = -1.66 x 10 3 J – 1.9 x 10 3 J = -240 J C = -q cu - q water / Δ T C = -240 J / 7.5 © = -32 J/©
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Sample Calculations Part B 11 and 12: 11. Heat evolved by reaction q HCl = 4.18 J/(g . ©) x mass of HCl solution in g x (T f – T i ) © q calorimeter = -q cu - q water q NaOH = 4.18 J/(g . ©) x mass of NaOH solution in g x (T
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This note was uploaded on 02/16/2011 for the course CHEM 101 taught by Professor Stegemiller during the Spring '07 term at Ohio State.

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Experiment 11 - Experiment 11: Calorimetry and Hesss Law...

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