A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization curve is 1.5x10^-4 mol/L. Calculate, in sequence, each of the following quantities in the aqueous solution to determine the equilibrium constant for the reaction:
Fe3+(aq) + SCN-(aq) <--> FeNCS2+(aq)
A) moles of FeNCS2+ that form in reaching equilibrium
B) moles of Fe3+ that react to form the FeNCS2+ at equilibrium
C) moles of SCN- that react to form the FeNCS2+ at equilibrium
D) moles of Fe3+ initially placed in the reaction system
e) moles of SCN- initially placed un the reaction system
f) moles of FE3+ (unreacted) at equilibrium
G) moles of SCN- (unreacted) at equilibrium
h) molar concentration of Fe3+ (unreacted) at equilibrium
i) molar concentration of SCN- (unreacted) at equilibrium
j) molar concentration of FeNCS2+ at equilibrium
k) Kc = [FeNCS2+]/([Fe3+][SCN-])