Lab Report10

Lab Report10 - Lab Report #10 Experiment: Chemical...

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Lab Report #10 Experiment: Chemical Equilibrium: Determination of an Equilibrium Constant Name: Lab Partner: Date Performed: 11/15/2008 Summary: In this experiment we need to find the equilibrium constant of a reaction. We need to make some calcula- tions and trials to find out the equilibrium constant. While we were doing experiment we observed the ef- fects of LeChatelier’s principle. Results: trial # [Fe 3+ ] i [Fe 3+ ] eq [SCN - ] i [SCN - ] eq [FeSCN 2+ ] eq K eq (K eq ) average 1 0.001 0.000958 0.0004 0.000358 0.000042 122 135 2 0.001 0.000931 0.0006 0.000531 0.000069 139 3 0.001 0.00091 0.0008 0.00071 0.00009 139 4 0.001 0.00089 0.001 0.00089 0.00011 139 Calculations: [Fe 3+ ] i = ml of [Fe(NO 3 ) 3 ]/(ml total)*0.002 M = 5 ml/(10 ml)*0.002 M = 0.001 M [SCN - ] i = ml of [KSCN]/(ml total)*0.002 M = 2 ml/(10 ml)*0.002 M = 0.004 M [FeSCN 2+ ] eq = A eq /A std *[FeSCN 2+ ] std = (0.072/0.343)*(1 ml/10 ml)*(0.002 M) ≈ 0.000042 M [Fe 3+ ] eq = [Fe 3+ ] i - [FeSCN 2+ ] eq = (0.001 – 0.000042)M = 0.000958 M
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This note was uploaded on 03/25/2008 for the course CHEM 107 taught by Professor Generalchemforeng during the Spring '07 term at Texas A&M.

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Lab Report10 - Lab Report #10 Experiment: Chemical...

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