Question

1. A student mixes 5.00 mL 2.00 X 10~3 M Fe(NO3)3 with 5.00 mL 2.00 X 10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.20 X 10-4 M. Find Kc for the reaction Fe3+(aq) + SCN-(aq) (arrows) FeSCN2 (aq).Step 1. Find the number of moles Fe3+ and SCN- initially present. (Use Eq. 3.)________moles Fe3+; ________moles SCN-Step 2. How many moles FeSCN2+ are in the mixture at equilibrium? What is the volume of the equilibrium mixture? (Use Eq. 3.).__________mL; ________moles FeSCN2+How many moles of Fe3+ and SCN~ are used up in making the FeSCN2"1"?.__________moles Fe3+; _________moles SCN-Step 3. How many moles of Fe3+ and SCN- remain hi the solution at equilibrium? (Use Eq. 4 and the results of Steps 1 and 2.)_______molesFe3+ ________molesSCN-Step 4. What are the concentrations of Fe3*, SCN-, and FeSCN2+ at equilibrium? What is the volume of the equilibrium mixture? (Use Eq. 3 and the results of Step 3.)[Fe3+] = _______M; [SCN-] =_________ M; [FeSCN2*] = _________MmLStep 5. What is the value of Kc for the reaction? (Use Eq. 2 and the results of Step 4.)Kc=_________