Experiment 6

Experiment 6 - DETERMINING AN EQUILIBRIUM CONSTANT The Concept of Chemical Equilibrium(Le Chateliers Principle pp 623 Textbook Chapter 14 Discuss

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DETERMINING AN EQUILIBRIUM CONSTANT The Concept of Chemical Equilibrium (Le Chatelier’s Principle) pp 623 Textbook Chapter 14 Discuss the same reaction of Experiment 6 Precision: Standard deviation from the mean Accuracy: % of Error Recitation February 28 1
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DETERMINING AN EQUILIBRIUM CONSTANT Recitation February 28 2 Fe(III) forms a complex with the thiocyanate (SCN - ) ion. The objective of this experiment is to determine the equilibrium constant (K) for the complex reaction: Fe 3+ (aq) + SCN - (aq) Fe(SCN) 2+ (aq) eq eq 3 eq 2 ] SCN [ ] Fe [ ] ) SCN ( Fe [ K - + + = Ten experiments will be run with different initial amounts of Fe 3+ and SCN - . The concentration of the complex ( [Fe(SCN) 2+ ] eq ) will be determined using spectrophotometry. Then, [Fe 3+ ] eq = [Fe 3+ ] initial – [Fe(SCN) 2+ ] eq and [SCN - ] eq = [SCN - ] initial – [Fe(SCN) 2+ ] eq The equilibrium constant is given by the expression =
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Recitation February 28 3 Preparation of the standard curve. (Determining k in Beer’s Law pp241 Prepare solutions with known amounts of complex.
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This note was uploaded on 05/01/2011 for the course CHEM 112 taught by Professor Hibbard during the Spring '08 term at Spelman.

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Experiment 6 - DETERMINING AN EQUILIBRIUM CONSTANT The Concept of Chemical Equilibrium(Le Chateliers Principle pp 623 Textbook Chapter 14 Discuss

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