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will like if answered fast and full
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Calibration curve Input the absorbances measured at 447 nm for the standard solutions 1−4. Plot a graph of absorbance ( y axis) vs concentration ( x axis), and add a linear trendline. Use the equation of the line to determine concentrations of [FeSCN]2+ corresponding to the absorbances for each unknown (1−5) in the table below. These are equilibrium concentrations of [FeSCN]2+. Unknowns Calculation of initial concentrations of reactants in unknowns Use M1​ V1​=M2​ V2​ 1min​=v2​V2​ (2×10−3)(5)=m2​(10) m2​=(2×10−2)(5)=.000 M1​= Concentration of reagent added to reaction mixture V1​= Initial volume of reagent added V2​= Total volume of reaction mixture M2​= Initial concentration of reagent in reaction mixture Determine the initial concentrations of Fe2+ and HSCN in the initial reaction mixtures of unknowns 1− 5. Input these concentrations on the chart provided below. Show calculations for the initial concentration, M2​, of Fej+ and HSCN in unknown 2 .
Data for determination of the equilibrium constant Equilibrium constant Average Kc​= Complete the table above using ICE diagrams to calculate K values. You need only show work for the calculation of K for unknown 1 . Calculation of the equilibrium constant for unknown 1 (Show ICE diagram).
1. Do the results support the equilibrium concept, as described. Explain. 2. In a Fe3+,HSCN equilibrium system at 24∘C it is found that [Fe3+]=1.85×10−4M,[HSCN]= 1.85×10−4M and [H+]=0.50M. Use your average value for the equilibrium constant to determine the concentration of FeSCN2 in the solution. 3. Why is the concentration of H+considered to be constant at 0.5M throughout the reaction. Is this strictly true?