What are the two half-reactions for the basic oxidized-reduction reaction Fe(OH)2+ H2O2 --> Fe(OH)3?
If I can find out the two half-reactions, I'll be able to balance the equation myself. Thanks!
Fe(OH)2 --> Fe(OH)3
H2O2 --> OH-
To determine the two half-reactions for the given oxidation-reduction (redox) reaction, we need to first identify the species being oxidized and reduced.
In this reaction, Fe(OH)2 is being oxidized to Fe(OH)3, which means it is losing electrons and undergoing an oxidation process. H2O2 is being reduced to O2, which means it is gaining electrons and undergoing a reduction process.
Now, let's break down the reaction into its two half-reactions:
1. Oxidation Half-Reaction:
Fe(OH)2 → Fe(OH)3
The Fe in Fe(OH)2 changes from a +2 oxidation state to +3 in Fe(OH)3. This means that Fe is losing an electron, so we can represent the oxidation half-reaction as:
Fe(OH)2 → Fe(OH)3 + e-
2. Reduction Half-Reaction:
H2O2 → O2
The oxygen in H2O2 is changing its oxidation state from -1 to 0 in O2. This means that the oxygen is gaining electrons, so we can represent the reduction half-reaction as:
H2O2 + 2e- → O2
Now that you have the two half-reactions:
1. Oxidation Half-Reaction: Fe(OH)2 → Fe(OH)3 + e-
2. Reduction Half-Reaction: H2O2 + 2e- → O2
You can then balance the equation by multiplying the half-reactions by appropriate coefficients to ensure that the number of electrons gained in the reduction half-reaction equals the number of electrons lost in the oxidation half-reaction.