Experiment 17.docx - Experiment 17 Chemical Equilibrium and...

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Experiment 17Chemical Equilibrium and Beer’s LawSeptember 29th, 2017 CHEM 1212KSection B05TA: Iramofu DominicHonor Pledge – Freshman Chemistry LaboratoriesI did not copy any portion of this work from the work of other students,old lab reports, or unreferenced materials. I understand that such activityis a violation of the Georgia Tech Honor Code.______________________________________SignatureAbstract
The purpose of this lab is to understand the chemical equilibrium (the point when the forward and reverse reactions happen at the same rate leaving the concentrations constant), the relationship between absorbance and concentration of a colored product, Fe(SCN)2+, using Beer’s law and spectroscopy. We made sure our reactions reached equilibrium by either very small amounts of one reactant relative to the other to assure its complete reaction or by leaving the mixtures for 10 minutes or more. Beer’s law indicates that the relationship between concentration and absorbance should be linear – this was verified by Part A of the experiment where the concentration of Fe(SCN)2+is known thanks to the complete reaction of the reactant Fe3+. Plotting the concentration with the experimentally determined absorbance did yield a linear graph with an R2value > 0.99. We were able to apply Beer’s law in a reverse manner to determine the concentrations of the product and remaining reactants given absorbance in Part B – these absorbance values were subsequently used to calculate product concentrations by working backwards with Beer’s law to determine the equilibrium constants. The equilibrium constant is expected to be constant as we run reactions

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