Determining the Equilibrium Constant for a Chemical Reaction

Determining the Equilibrium Constant for a Chemical...

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Lab 3 Determination of an Equilibrium Constant for a Chemical Reaction Sonya Dhanjal Student # 1055144 Lab Partner: Jamal Farooq Student # 0945659 McMaster University Chemistry 1A03 L65 TA: Lauren Conducted: Wednesday November 3, 2010 Due: Wednesday November 10, 2010 Purpose
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To ultimately determine the equilibrium constant of iron (III) thiocyanate, FeSCN 2+ . This will be done by mixing various concentrations of the reactants iron(III) nitrate, Fe(NO 3 ) 3 , and potassium thiocyanate, KSCN - , and then using spectrometry to relate the absorbency of the product, FeSCN 2+ , to its concentration. Procedure Please refer to the 2010 Chemistry 1A03/1E03 Lab Manual for detailed procedure under, Determination of an Equilibrium Constant for a Chemical Reaction. No changes were made. Results note that spectrophotometer wavelength was set to 447nm for entire lab Part A Data for each flask in Part A Flask Volume of 0.002M KSCN - (mL) Volume of 0.200M Fe(NO 3 ) 3 (mL) Absorption Value 1 0.001 0.049 0.237 2 0.002 0.048 0.416 3 0.003 0.047 0.628 Calculations SCN - (aq) + Fe 3+ (aq) FeSCN 2+ (aq) Flask 1 [FeSCN 2+ ] e = [SCN - ] i Flask 2 [FeSCN 2+ ] e = [SCN - ] i Flask 3 [FeSCN 2+ ] e = [SCN - ] i
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Part B Data for each test tube in Part B Test Tube Volume of 0.002M KSCN - (L) Volume of 0.002M Fe(NO 3 ) 3 (L) Volume of H 2 O (L) Absorption Value 1 0.001 0.005 0.004 0.105 2 0.002 0.005 0.003 0.221 3 0.003 0.005 0.002 0.348 4 0.004 0.005 0.001 0.445 5 0.005 0.005 --- 0.546 Calculations
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note that all FeSCN 2+ equilibrium concentration values were interpolated from “Concentration of FeSCN 2+ vs. Absorbance” graph from Part A Test Tube 1 Discussion
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This note was uploaded on 02/26/2011 for the course CHEM 1a03 taught by Professor Landry during the Fall '08 term at McMaster University.

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Determining the Equilibrium Constant for a Chemical...

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