Students should be able to: The equilibrium constant The law of mass action expresses the relative concentrations of reactants and products in terms of a quantity called Keq. The value of Keq is only affected by temperature. Changes in concentrations do not affect Keq.
The purpose of this experiment is to calculate the equilibrium constant for the reaction of iron III ions with thiocyanate ions.
Chemical equilibrium occurs when both forward and reverse reactions proceed at the same rate, and the concentrations of the products and reactions are the same.
Write the equilibrium constant expression for the reaction.
Calculate the value of the equilibrium concentration of NH3 uncomplexed. Calculate the value of the equilibrium constant. Standard Volume of 0. Use the dilution equation to calculate the concentration of SCN- ions in the five reference solutions before any reaction occurs.
See Data Table 3 6 Use Equation 4 in the background section to calculate the value of the equilibrium constant Keq for each test solution See Data Table 3 7 Calculate the mean of the equilibrium constant for the five test solutions.
See Data Table 3 8 Calculate the average deviation for Keq. See Data Table 3 9 The average deviation describes the precision of the results.
The average deviation indicates that the equilibrium constant is indeed constant. Fingerprints on the cuvets could have affected the outcome, as well as any other contaminants that may have gotten onto them.
Was the value constant for all your experiments? Should it be constant? The equilibrium should be constant with all of the concentrations of the components involved in the reaction.
The values were generally constant for all of the experiments, with some experimental error. In other words, at equilibrium, are there mostly products, reactants, or relatively large amounts of both? The value of Keq determines whether a reaction is product or reactant favoring.
|Writing a formal lab report||Lab report for keq of fescn Adlai December 27, Are sample research, students have been supplied contains the reaction from the fe scn. Determination of fescn2 ion, fescn2 lab reports like this experiment, buy essay sample determination of keq for the colorimeter shown in this essay sample lab report.|
In this experiment, the equilibrium constants were relatively large, at well over 1. As a result, there are mostly products. A spectrophotometer measures the amount of light that can pass through a given substance. We could thus use the absorbances of light to create a function that can be used to solve for the unknowns.
What was the color of light chosen for this experiment? The spectrophotometer should not be set to a wavelength of light to the same color as the solution, because the light would be reflected back and not absorbed. This would not give accurate or favorable experimental results.
What is the major source of error in the experiment? The numbers attained from the spectrophotometer can be as precise to the thousandths place. The major source of error from the experiment would be substances accidentally coated on the cuvet that could block or absorb light.
A spectrophotometer could be useful in indicating slight changes in color to a solution that may be going through a chemical reaction.Determination of the Equilibrium Constant for Ferric Thiocyanate To learn about Chemical Equilibrium.
To learn about the Ferric Thiocyanate system. To learn about Absorbance Spectroscopy. In this laboratory exercise, we will determine the Equilibrium Constant for the reaction between.
Experiment 8 Determination of an Equilibrium Constant OUTCOMES After completing this experiment, the student should be able to: use absorbance data to find the concentration of a .
Determination of an Equilibrium Constant Minneapolis Community and Technical College Principles of Chemistry II, C v I. Introduction Equilibrium Consider the following situation: It is rush hour and cars are entering the I freeway at a rate of 30 cars per second.
determination of the Equilibrium Constant for the formation of FeSCN2+ Fe3+ + SCN- FeSCN2+ The equilibrium concentration of FeSCN 2+ was x 10^-4 M Calclulate the equilibrium constant for the reaction. I got The equilibrium constant, Keq, is defined . Determination of an Equilibrium Constant Minneapolis Community and Technical College Principles of Chemistry II, C v I. Introduction Equilibrium Consider the following situation: It is rush hour and cars are entering the I freeway at a rate of 30 cars per second. Obviously, if. The Determination of Keq for FeSCN2+ Objective: The purpose of this experiment is to calculate the equilibrium constant for the reaction of iron(III) ions with thiocyanate ions. Pre-Lab Questions: 1) Define equilibrium. Chemical equilibrium occurs when both forward and reverse reactions proceed at the.
Obviously, if. View Notes - Ch LAB-Determination of Keq for FeSCN Key from CHEM at Curie Metropolitan High School. Data Tables Data Table 1 Reference%(23). The Determination of K eq for FeSCN 2+. A chemical system is said to be in equilibrium when there are no measurable changes occurring.
An example of . FeSCN2+ for any of the equilibrium systems can be found by: [FeSCN2+]eq = Aeq Astd X [FeSCN 2+]std Knowing the [FeSCN2+]eq allows you to determine the concentrations of the other two ions at equilibrium. For each mole of FeSCN2+ ions produced, one less mole of Fe3+ ions will be found.