Determination of Heat of Dissolution

Determination of Heat of Dissolution - Determination of...

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Determination of Heat of Dissolution (∆H dissolution ) of Potassium Chloride (KCl) Trial 1 Trial 2 Mass of KCl (0.001g) 1.019g 1.019g Mass of calorimeter (0.001g) 8.226g 8.419g Mass of calorimeter and water (0.001g) 33.117g 33.253g Mass of water (0.001g) 24.891g 24.834g Mass of solution (0.001g) 34.154g 33.953g Initial temperature of water (0.01ºC) 22.5°C 20.8°C Final (equilibrium) temperature of system (0.01ºC) 18.8°C 18.64°C File names 119 120 Calculations 34.117g – 8.226g = 25.891g water 33.253g – 8.419g = 24.834g water Calculation of (∆H dissolution ) Trial 1 -q reaction = ( m solution x C solution x ΔT solution ) + (C calorimeter x ΔT solution ) = (1.019g x 4.184J/gºC x (-3.70 ºC)) + (13.8J/ºC x (-3.70 ºC)) = (-15.77J + -51.6J) ΔT solution = 18.8 ºC – 22.5 ºC = -3.70 ºC = 67.37 J x 1 kJ /1000 J = .06737 kJ Molar mass KCl = 39.0983 g/mol + 35.453 g/mol = 74.5513 g/mol 1.019g KCl x 1 mol / 74.5513g KCl = .013668 mol KCl ΔH Dissolution = q reaction ( kJ ) / moles of limiting reactant = .0673
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This note was uploaded on 03/17/2009 for the course CHEML 1212 taught by Professor Anderson during the Spring '08 term at UGA.

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Determination of Heat of Dissolution - Determination of...

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