1. Explain why the actual coefficients of the ferrous ammonium sulfate hexahydrate and the potassium iron oxalate complex in the balanced equation describing the overall process are not required for computing the predicted weight of the product.
2. Balance each of the following equations:
a. Fe(NH4)2 (SO4)2 •6H20 (aq) + H2C2O4 (aq) → FeC204 2H20 (s) + NH4HSO4 (aq) + H20
b.FeC204*2H20 (s) + H2O2 (aq) + K2C2O4 (aq) → [Fe(C2O4)3]3- (aq) + K+ (aq) + OH- (aq) + H2O a Note that the reaction given in part b. is a redox process. You must use the half-reaction method to balance this reaction.
c. [Fe(C2O4)3]- (aq) + K+ (aq) + H20 → K3Fe(C204)3 3H20 (s)
3. Assuming that ferrous ammonium sulfate hexahydrate is the limiting reagent in the process described in question 2, compute the theoretical amount of product formed from 1.00 g of Fe(NH4)2 (SO4)2 •6H2O.
4. A student used 2.50 g of Fe(NH4)2 (SO4)2 •6H20 as starting material for the process described in this experiment. She obtained 2.95 g of the product, K3Fe(C2O4)3•3H20. Compute the percentage yield of this student’s preparation. Show the equation used before inserting the values.