To answer the question here is problem 1 thank you:

2. Optional Assume that the reaction studied in Problem I is Fe3 (aq) +2SCN(aq )=Fe2(SCN22 (aq). Find Kc for this reaction. given the data in Problem 1. a. Formulate the expression for Ke for the altemate reaction just cited. b. Find Kv as you did in Problem I: take due account of the fact that two moles SCNare used up per mole Fe(SCN))2 formed as you carry out the calculations on the temainder of this pigge: Step 1 Results are as in Problem 1. Step 2 How many moles of Fe(SCN2+are in the mixture at equilibrium? (This will be the same as your answer for Step 2 in Problem 1.) How many moles of Fe3+ and SCNare used up in making the Fe(SCN )2+? moles Fe(SCN2)2 1. A student mixes 5.00mL of 2.00103MFe2(NO3), in 1.0MHNO3 with 4.00mL of 2.00103MKSCN and 1.00mL of water. He finds that in the equilibrium mixture the concentration of FeSCN FN2+ is 7.0105M. Find Kc for the reaction Fe1+(aq)+SCN(aq)=Fe(SCN)2+(aq). Step 1 Calculate the number of moles Fe3+ and SCNinitially present. (Use Eq. 3.) Fe3t02103510001=1105molSCN0:2103310001=6106mol105molesFe34:8106molesSCN at equilibrium? (Use Eq. 3.) How many moles of Fe3+ and SCNare used up in making the FeSCN2+ ? (7105)(90)(10001)=455107mol 4107molesF3:4107molesSCN Step 3 How many moles of Fe3+ and SCNremain in the solution at equilibrium? (Use Eq. 4 and the Step 4 What are the concentrations of Fe1+. SCN, and FeSCN2+ at equilibrium? (Use Eq. 3 and the Step 5 What is the value of Kc for the reaction? (Use Eq. 2 and the results of Step 4.) Kc=[Fe3+][SCN][Fe(SCN)2+]=(1.1103)(8.4104)4.5107=489