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1. FeSO4∙(NH4)2SO4∙ 6H2O + H2C2O4∙ 2H2O ---> FeC2O4 + (NH4)2SO4 + H2SO4 + 8H2O 2. 6 FeC2O4 + 3H2O2 + 6K2C2O4∙ H2O ---> 4 K3[Fe(C2O4)3]∙ 3 H2O + 2 Fe(OH)3 + 6 H2O 3. 2 Fe(OH)3 + 3 H2C2O4∙
1.
FeSO4∙(NH4)2SO4∙ 6H2O + H2C2O4∙ 2H2O ---> FeC2O4 + (NH4)2SO4 + H2SO4 + 8H2O
2.
6 FeC2O4 + 3H2O2 + 6K2C2O4∙ H2O ---> 4 K3[Fe(C2O4)3]∙ 3 H2O + 2 Fe(OH)3 + 6 H2O
3.
2 Fe(OH)3 + 3 H2C2O4∙ 2H2O + 3 K2C2O4∙ H2O ----> 2 K3[Fe(C2O4)3]∙ 3H2O + 9 H2O
In this experiment 4.0g of ferrous ammonium sulphate is used. assuming everything else is added in excess; calculate the theoretical yield of the iron complex. Work through the entire reaction sequence; do not simply assume the number of moles of limiting reaction equals the number of moles of your final product.
