Given the Following data at 298K,

Fe3+ + SCN- = FeSCN2+

5.00mL of 0.002 M Fe3+ was combined with 3.00mL of 0.002 M SCN- at 2.00mL of 1.0M HNO3 at 298k. The resulting solution had an absorbance of 0.11 at 440nm and Kc=2.34x10^3 m^-1. Determine the equilibrium constant for FeSCN2+. (Hint: use A=Kc(C) to determine the equilibrium concentrations of the reactants and then set up an equilibrium expression to calculate the Keq

Question

Given the Following data at 298K, 

Fe3+ + SCN- = FeSCN2+

5.00mL of 0.002 M Fe3+ was combined with 3.00mL of 0.002 M SCN- at 2.00mL of 1.0M HNO3 at 298k. The resulting solution had an absorbance of 0.11 at 440nm and Kc=2.34x10^3 m^-1. Determine the equilibrium constant for FeSCN2+. (Hint: use A=Kc(C) to determine the equilibrium concentrations of the reactants and then set up an equilibrium expression to calculate the Keq