how do u do a redox balance of the following reaction : Fe(NH4)2(SO4)2*6H2O + H2C2O4 + K2C2O4 + H2O2 -> K3Fe(C2O4)3*3 H2O + (NH4)2SO4 + H2SO4 +H2O
i only know Fe2+ -> Fe3+ +1e-
The O in the peroxide is -1, but in the product side, all O are -2, so O-1 gains an electron.
Just as an aside here, I believe you have omitted something from the equation (or perhaps you made a typo) BUT there is no Fe on the left and you have Fe on the right. Something is amiss
To balance the redox reaction, you need to follow a few steps. First, identify the oxidation states of all the elements in the reaction. Then, assign a coefficient to each compound to balance the number of atoms on each side of the equation. Finally, balance the charges and electrons to ensure charge conservation.
Step 1: Identify the oxidation states
In Fe(NH4)2(SO4)2*6H2O, the oxidation state of Fe is +2. In Fe3+, the oxidation state is +3 (as you mentioned).
In H2C2O4 (oxalic acid), the overall oxidation state is 0 since it is a neutral compound.
In K2C2O4 (potassium oxalate), the oxidation state of K is +1, and of the C2O4 group is -2.
In H2O2 (hydrogen peroxide), the oxidation state of H is +1, and of O is -1.
In K3Fe(C2O4)3*3H2O, the oxidation state of K is +1, and of Fe is assumed to be +3 (to balance the overall charge). The oxidation state of the C2O4 group is -2.
In (NH4)2SO4 (ammonium sulfate), the oxidation state of N is -3, of H is +1, of S is +6, and of O is -2.
In H2SO4 (sulfuric acid), the oxidation state of S is +6, and of O is -2.
In H2O (water), the oxidation state of H is +1, and of O is -2.
Step 2: Assign coefficients to balance the number of atoms
In the reaction, the coefficients are:
Fe(NH4)2(SO4)2*6H2O + H2C2O4 + K2C2O4 + H2O2 -> K3Fe(C2O4)3*3 H2O + (NH4)2SO4 + H2SO4 + H2O
1 + 1 + 1 + 1 -> 1 + 1 + 1 + 6
Step 3: Balance the charges and electrons
In this step, you need to balance the charges and the number of electrons to ensure charge conservation. For example, if there's an increase in charge on one side of the equation, you balance it with an equal decrease in charge on the other side.
Let's focus on the iron (Fe) atoms:
Fe2+ -> Fe3+ + 1e-
On the left side, there is 1 Fe2+ atom, while on the right side, there is 1 Fe3+ atom. Therefore, you need to multiply the left side of the equation by 1 to balance the number of Fe atoms.
The balanced equation becomes:
Fe(NH4)2(SO4)2*6H2O + H2C2O4 + K2C2O4 + H2O2 -> K3Fe(C2O4)3*3 H2O + (NH4)2SO4 + H2SO4 + H2O
I hope this helps you in balancing the redox reaction! Let me know if you have any further questions.