Please help answer the questions for the calculations part it is the last 3 page
ID: 702084 • Letter: P
Question
Please help answer the questions for the calculations part it is the last 3 pages. I am really stuck I put my results for the data table part 1 and2.ASAP please thank you!!!! This is the full report please don’t say more infoThe Determination of an Equilibrium Constant The equilibrium state of a chemical reaction can be characterized by quantitatively defini equilibrium constant, Keg. In this experiment, you will determine the value of Keg for the react between iron (III) ions and thiocyanate ions, SCN Fe (aq)+ SCN (aq) FesCN (aq) When you mix amounts of Fe3 and SCN, a reaction occurs to produce FeSCN, but ts react. Thus, your beaker (or flask or cauldron) will contain some of each of these three species, which is your e figure out a way to count the number of different ions in the reaction mixture. That is the ma objective of this experiment, and to achieve this objective you will take advantage o about FeSCN2+-in aqueous solution it has a reddish color. The two reactants. Fe3-and SCN quilibrium system. To learn more about the system, we need to f something are essentially colorless in solution, thus the red color you will see when you conduct the reaction is produced by the FeSCN ions. One of the more important numbers that help us understand an equilibrium sy equilibrium constant, Keg. For the reaction between Fe and SCN, the Key is defined by the equation shown below. stem is called the FeSCN [Fe IISCN To find the value of Keg at a given temperature, it is necessary concentration of each of the three species in solution at equil to determine the molar ibrium. You will determine the ncentrations by using a Vernier Colorimeter or Spectrometer to measure the amount of light o cific wavelength that passes through a sample of the equilibrium mixtures. The amount o light absorbed by a colored solution is proportional to its concentration. The red FeSCN olution absorbs blue light, thus the Colorimeter users will be instructed to use the 470 nm (blue) LED. Spectrometer users will determine an appropriate wavelength based on the absorbance spectrum of the solution. The wavelength will be close to, but not exactly, 470 nm In order to successfully evaluate this equilibrium system, it is necessary to conduct tw tests. In Part I of the experiment, you will prepare a series of standard solutions of Fes solutions of varying concentrations of SCN and constant concentrations of H and Fe that are in stoichiometric excess. The excess of H ions will ensure that Fe engages in no side reactions to form FeOH2, for example) which could interfere with your measurements. In an exces Fe ions, the SCN ions will be the limiting reagent, thus all of the SCN will form FeSCN2 ions. The FeSCN2+ complex forms slowly, taking at least one minute for the color to develop. It is best to take absorbance readings after a specific length of time has passed, between two four minutes after preparing the equilibrium mixture. Do not wait much longer than five minutes to take readings, however, because the mixture is light sensitive and the FeSCN ions will slowly decompose. rom In Part II of the experiment, you will prepare a new series of solutions that have varied concentrations of the SCN ions and constant concentrations of H ions and Fe ions. You will use the results of this test to accurately evaluate the equilibrium concentrations of each species and calculate the Key of the reaction.
Explanation / Answer
a) The readings for the Part 1 are incorrect, the data of concentration of [FeSCN]2+ Versus Absorbance should be approximately linear. That's how you would get a linear regression equation which will tell you how concentration varies as a function of absorbance. In think you will have to repeat the experiment for correct data. Once you have correct info, calculate the linear eauation relating absorbance and concentration and then in the second part from that equation, you can concentration at different absorbances. This you have to do for all different ions.
b) After that, you have to know where these are concentrations are converging, that will be equilibrium concentrations. From those concentrations, you can calculate equilibrium constant.