Suppose a student mixes 4.00 mL of 2.00 # 10-3 M Fe(NO3 ) 3 with 5.00 mL of 2.00 # 10-3 M KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be 8.75 # 10-5 M. Find the equilibrium constant for the following reaction. Show all your calculations for each step. Fe3+ (aq) + SCN- (aq) FeNCS2+ (aq) Step 1. Calculate the initial number of moles of Fe3+ and SCN- (use Equation 12). moles of Fe3+ moles of SCN- Step 2. How many moles of FeNCS2+ are present at equilibrium? What is the volume of the equilibrium mixture? mL moles of FeNCS2+ How many moles of Fe3+ and SCN- are consumed to produce the FeNCS2+? moles of Fe3+ moles of SCN-