# Suppose a student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO,)3 with 4.00 mL of 2.00 x 10-3 M KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be 9.25 X 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. 3/3 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 Step 3. Calculate the number of moles of Fe3+ and SCN- remaining at equilibrium. Use Equa- tion (13) and the results of Steps 1 and 2. moles of Fe3+ moles of SCN 9

Question

I have a 3 step problem about Determination of an Equilbrium constant. help_outlineImage TranscriptioncloseSuppose a student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO,)3 with 4.00 mL of 2.00 x 10-3 M KSCN and 1.00 mL of water. The student then determines the [FeNCS2+] at equilibrium to be 9.25 X 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. 3/3 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 Step 3. Calculate the number of moles of Fe3+ and SCN- remaining at equilibrium. Use Equa- tion (13) and the results of Steps 1 and 2. moles of Fe3+ moles of SCN 9 fullscreen

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