please answer and explain a, and b 1-5 thanks

A student mixes 5.00mL2.00e03M Fe(NO3)3 in 1.00M HNO3 with 3.00mL2.00e03M KSCN and 2.00mL of water. She finds that in the equilibrium mixture the concentration of Fe(SCN)2+is 7.00e05M For the equilibrium: Fe3+(aq)+2SCN(aq)Fe(SCN)2+(aq) a. Which of the following expressions for the equilibrium constant, Kc, for the above reaction, is correct? Kc=[Fe(SCN)2+][Fe3+][2SCN]Kc=[Fe(SCN)2+][Fe3+][SCN]2Ke=[Fe3+][2SCN]Fe(SCN)2+Ke=[Fe3+][2SCN]2[Fe(SCN)2+]Kc=[Fe3+][SCN]2[Fe(SCN)2+]Ke=[Fe(SCN)2+][Fe3+][2SCN]2 b. Follow the steps below to calculate Kc for this reaction. 1. Find the number of moles of Fe3+ and SCNinitially present. MolesA(mol)=MolarityofA(M)Volumeofsolution(L) MolesofFe3+initiallypresent=molesFe3+ Moles of SCNinitially present = moles SCN Moles of Fe3+ initially present = Moles of SCNinitially present =moles SCN 2. How many moles of Fe(SCN)2+are in the mixture at equilibrium? Moles of Fe(SCN)2+at equilibrium =moles Fe(SCN)2+ How many moles of Fe3+ and SCNare used up in making the Fe(SCN)2+. Moles of Fe3+ used up = moles Fe3+ Moles of SCNused up= moles SCN 3. How many moles of Fe3+ and SCNremain in solution at equilibrium? Moles SCNat equilibrium =Initial moles SCN(2MolesFe(SCN)2+) Moles of Fe3+ at equilibrium = moles Fe3+ Moles of SCNat equilibrium =moles SCN 4. What are the concentrations of Fe3+, SCN, and Fe(SCN)2+at equilibrium? Concentration of Fe3+ at equilibrium =M Concentration of SCNat equilibrium =M Concentration of Fe(SCN)2+at equilibrium =M 5. Calculate Kc Kc=