2Fe(NH 4 ) 2 (SO 4 ) 2 .6H 2 O+ 6K 2 C 2 O 4 +H 2 O 2 +H 2 SO 4 --------2K 3 [Fe

Question

2Fe(NH4)2(SO4)2.6H2O+ 6K2C2O4+H2O2+H2SO4 --------2K3[Fe(C2O4)3].3H2O+3K2SO4+2(NH4)2SO4+8H2O What is the oxidizing/reducing agent that is changing theoxidation state of the iron? 2Fe(NH4)2(SO4)2.6H2O+ 6K2C2O4+H2O2+H2SO4 --------2K3[Fe(C2O4)3].3H2O+3K2SO4+2(NH4)2SO4+8H2O What is the oxidizing/reducing agent that is changing theoxidation state of the iron?

Explanation / Answer

The easiest way to do this is by assigning the oxidation numbers toeach element in the compounds. Because the coefficient doesn'tmatter, I'm going to ignore those when retyping the equation. Forpolyatomic ions, instead of writing out the oxidation number forevery element, I will just type out the overall charge to keep thisfrom looking too cluttered. +3 2(+1) 2(-2) 2(+1)-2 2(+1) -2      +1 -1 2(+1) -2   3(+1) +3 3(-2) 2(+1) -2 2(+1) -2 2(+1)    -2 2(+1) -2 Fe(NH4)2(SO4)2.6H2O+ K2C2O4+H2O2+H2SO4 -->K3[Fe(C2O4)3].3H2O+K2SO4+(NH4)2SO4+H2O The two elements that change oxidation states are Iron (Fe) and theOxygen in H2O2. +3                                                  -1                         +2                                                                   -2 Fe(NH4)2(SO4)2.6H2O+ K2C2O4+H2O2+H2SO4 -->K3[Fe(C2O4)3].3H2O+K2SO4+(NH4)2SO4+H2O Iron becomes less positive, so it's gaining electrons, therefore itis reduced. So the Hydrogen Peroxide is the oxidizing agent that reducesIron.

Related Questions

Navigate

• Browse (All)
• Browse 2
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.