When h2o2 and dilute h2so4 are added to feso4 what substance undergoes oxidation and reduction
In the reaction between H2O2 and dilute H2SO4 with FeSO4, FeSO4 is oxidized and H2O2 is reduced.
Write half equation when h2o2 undergo reduction
The half equation for the reduction of H2O2 can be written as:
H2O2 + 2H+ + 2e- -> 2H2O
When H2O2 and dilute H2SO4 are added to FeSO4, the substance that undergoes oxidation is H2O2 (hydrogen peroxide) and the substance that undergoes reduction is FeSO4 (iron(II) sulfate).
To explain it step-by-step:
1. H2O2 (hydrogen peroxide) is a strong oxidizing agent, meaning it can readily donate oxygen or accept electrons from other substances.
2. FeSO4 (iron(II) sulfate) is a compound containing Fe2+ ions. Fe2+ can readily be oxidized to Fe3+.
3. When H2O2 is added to FeSO4 in the presence of dilute H2SO4 (sulfuric acid), the following reaction takes place:
H2O2 + FeSO4 + H2SO4 → Fe2(SO4)3 + H2O
In this reaction, H2O2 donates oxygen to the Fe2+ ions, causing the Fe2+ ions to be oxidized to Fe3+ ions. This is the oxidation step.
At the same time, the H2O2 is reduced as it accepts electrons from Fe2+ ions, becoming water (H2O). This is the reduction step.
Thus, in this reaction, H2O2 undergoes oxidation, while FeSO4 undergoes reduction.
To determine which substance undergoes oxidation and reduction when H2O2 (hydrogen peroxide) and dilute H2SO4 (sulfuric acid) are added to FeSO4 (iron(II) sulfate), we need to examine the changes in oxidation states of the elements involved.
First, let's write the balanced chemical equation for the reaction:
FeSO4 + H2O2 + H2SO4 → ?
In this reaction, FeSO4 is composed of the Fe2+ ion and SO4^2- ion. H2O2 breaks down into H2O and O2, and H2SO4 dissociates into H+ and SO4^2- ions.
Now, let's consider the potential oxidation states of the elements involved:
- Iron (Fe) can have oxidation states of +2 (in FeSO4) and +3 (in Fe2(SO4)3).
- Sulfur (S) can have oxidation states of -2 (in FeSO4 and SO4^2-) and +6 (in H2SO4).
- Oxygen (O) usually has an oxidation state of -2 but can have other oxidation states such as -1 (in H2O2) or 0 (in O2).
By examining the reaction equation, we see that the Fe2+ ion in FeSO4 is being oxidized to Fe3+. This means it is losing electrons and increasing its oxidation state from +2 to +3. Therefore, Fe2+ is undergoing oxidation.
On the other hand, the H2O2 molecule is being reduced to form H2O. This means it is gaining electrons and decreasing its oxidation state. In this case, the oxygen atom in H2O2 is changing its oxidation state from -1 to -2, which indicates reduction.
So, in the reaction between FeSO4, H2O2, and H2SO4, Fe2+ in FeSO4 undergoes oxidation, while H2O2 undergoes reduction.