Chemical Equilibrium Lab Report

Bianca Furci 3/9/17
E4 Professor Kiwiett A Study of Chemical Equilibrium The goal of the experiment was to determine the equilibrium constant of the equation between the reaction:

[1]
Assuming that SCN– was the limiting reactant, and that essentially all of it was used up to make FeSCN2+. In equation 1, it was known that the product, FeSCN2+ was the most intensified ion relating to light absorbance. By doing this, it was possible to equate the equilibrium concentration of iron (III) thiocyanate, [FeSCN2+] eq to the initial concentration of thiocyanate, [SCN−]initial. In order to determine the known values of K, the maximum wavelength of this product has to be calculated because it’s relative to its concentration. A

The accepted range of k according to a comparative study at the University of Alaska Fairbanks was 130-280. This proves that our k value was valid because it falls within this range proving that our reaction had a higher intensity since it was closer to the value of 280.
[3]
The average of these values was calculated by adding all values and dividing that number by six. The number was the state in which the reactants and products have no net change over time, and the forward and reverse reactions are at equal rates. This is the equilibrium constant resulting from the combination of iron(III), Fe3+ ion and thiocyanate, SCN- ion that creates [FeSCN2+].
All in all, the experiment was validated because it showed the expected results that as concentration increased, so did the absorption of the reaction. The purpose of the experiment was proven by comparing certain concentrations and their ability to reach a rate of