Fe3+ is reduced to Fe2+ by using
2Fe+3 + H2O2 + 2OH– → 2Fe+2 + 2H2O + O2
Na2O2 + H2O → H2O2 + NaOH
This question involves understanding redox reactions where Fe3+ is reduced to Fe2+. Let's analyze the concept step by step:
Step 1: Identify the Reduction Process
Reduction means gain of electrons. The half-reaction is:
So, we need a reducing agent that can donate electrons to Fe3+.
Step 2: Analyze the Options
Both Na2O2 and H2O2 can act as oxidizing or reducing agents depending on the medium. In acidic medium, H2O2 acts as a reducing agent. The relevant reaction is:
Here, H2O2 is oxidized to O2, donating electrons, which can reduce Fe3+ to Fe2+.
In basic medium, H2O2 typically acts as an oxidizing agent. Na2O2 in water gives NaOH and H2O2, creating a basic medium, which is not suitable for reduction of Fe3+.
Step 3: Determine the Correct Option
Thus, H2O2 in acidic medium (H2SO4) acts as a reducing agent and can reduce Fe3+ to Fe2+. The other options either provide basic conditions or use Na2O2 which may not be effective.
Final Answer: H2O2 in presence of H2SO4
Redox Reactions: Reactions involving transfer of electrons between species. oxidizing agents accept electrons, reducing agents donate electrons.
Hydrogen Peroxide Properties: H2O2 can act as both oxidizing and reducing agent. In acidic medium, it is a good reducing agent for strong oxidizing agents.
Reduction half-reaction:
Oxidation half-reaction for H2O2 in acid: