CHEMISTRY Chemical Equilibrium

CHEMISTRY Chemical Equilibrium - William Pit t man Chemist...

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William Pittman Chemistry 12 – 3 -07 Lilly Chemical Equilibrium In this experiment, we attempted to evaluate the equilibrium constant from certain reactions. In order to evaluate the equilibrium constant, we made 4 different coalition using different amount of each variable liquid and also a standard solution which is of a much higher absorbance. These 4 solutions were place in a colorimeter and their transparency and absorbency values were recorded. As we increased the amount of KSCN and decreased the amount of water, the solution developed a higher absorbance and less transparency (these go hand in hand). Calculations : Initial Concentration of Fe 3+ : [ Fe +] 3 = ( [ ( ) ] / ) . i mL of Fe NO3 3 mL total x 0020 M [ Fe +] 3 = ( / ) . i 5 mL 10 mL x 0020 M [ Fe +] 3 = . i 001 M Initial Concentration of SCN - : [ SCN -] = ( / ) . i mL of KSCN mL total x 0020 M [ SCN -] ( ) = ( / ) . i trial one 2 mL 10 mL x 0020 M [ SCN -] ( ) = i trial one 4 x 10 - 4 M [ SCN -] ( ) = i trial two 6 x 10 4 M [ SCN -] ( ) = i trial three 8 x 10 4 M
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[ SCN -] ( ) = . i trial four 001 M Calculating [FeSCN 2+ ] eq : [ FeSCN +] 2 = ( / ) [ eq Aeq Astd x FeSCN +] 2 std [ FeSCN +] 2 ( ) = (. / . ) . eq trial one 032 690 x 00020 [ +] FeSCN2 ( ) = . eq trial one 9 28 x 10 - 6 [ +] FeSCN2 ( ) = . eq trial two 2 46 x 10 - 5 [ +] FeSCN2 (
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This note was uploaded on 03/19/2011 for the course CHEM 107 taught by Professor Generalchemforeng during the Spring '07 term at Texas A&M.

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CHEMISTRY Chemical Equilibrium - William Pit t man Chemist...

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