Experiment 14 Equilibrium Constant

Experiment 14 Equilibrium Constant - Experiment 14 –...

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Unformatted text preview: Experiment 14 – Determination of an Equilibrium Constant Summer 2010 Name TD Khang Lab Section 409 Point Summary (See Blackboard for detailed grading rubric) Superior Excellent Satisfactory Fair Poor Omitted Introduction •Purpose of Report •Goals of Experiment Materials and Methods Results and Discussion •Description of data •Data Tables •Data Table Titles •Graphs •Figure Captions •Sample Calculations •Systematic Error •Random Error •Discussion of discrepancies Other Lab Technique TOTAL POINTS TA Comments/Suggestions: C HEMISTRY 102L R EPORT T EMPLATE EXPT. Determination of an Equilibrium Constant 14 14 Introduction The purpose of this experiment is to understand the idea of chemical equilibrium by learning how to determine the equilibrium constant (Kc) for a reaction in solution. The goals of the experiment are to create a standard curve for Absorbance versus Concentration of a reaction. The concentration of a specific reaction can be determined using the Beer-Lambert, the absorbance of the solution, and the standard curve. The equilibrium concentrations of the remaining reactions can be determined using the equilibrium concentration determined from Beer-Lambert Law, and the initial concentrations in the ICE method. The main purpose for calculating initial and equilibrium concentrations in a reaction is to be able to evaluate the change in concentration in order to determine all equilibrium concentrations. The final equilibrium constant can be determined from the calculated equilibrium concentrations by dividing the product of the products’ equilibrium concentrations by the reactants’ equilibrium concentrations. Materials and Methods The procedure for this experiment was taken from the experiment 14 lab manual in the CHEM 102 lab folder at the University of North Carolina at Chapel Hill in the fall semester of 2010. Some deviations from the procedure did occur. The amount of reactant weighed and used wasn’t exactly the same as the amount required by the procedure. The use of incorrect significant figures could have led to less or more precise calculated data. Calculation errors may have also occurred thus giving incorrect answers. The calibration of the colorimeter may have been off thus it would provide skewed data. calibration of the colorimeter may have been off thus it would provide skewed data....
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This note was uploaded on 02/29/2012 for the course BIO 101 taught by Professor Desaix during the Spring '11 term at UNC.

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Experiment 14 Equilibrium Constant - Experiment 14 –...

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