How many electrons are transferred in the reaction of hydrogen peroxide with iron (II) ion in
acidic solution to form iron (III) ion and water
Going from Fe++ to Fe+++ involves the loss of ONE electron per Fe Ion
To determine the number of electrons transferred in a chemical reaction, you need to balance the oxidation-reduction (redox) equation. The balanced redox equation will provide you with the stoichiometric coefficients of the species involved in the reaction, which can be used to determine the number of electrons transferred.
The overall balanced redox equation for the reaction between hydrogen peroxide (H2O2) and iron (II) ion (Fe2+) in acidic solution to form iron (III) ion (Fe3+) and water (H2O) is as follows:
2 Fe2+(aq) + H2O2(aq) + 2 H+(aq) → 2 Fe3+(aq) + 2 H2O(l)
In this equation, the iron (II) ions are oxidized from a +2 oxidation state to a +3 oxidation state, while hydrogen peroxide is reduced from a 0 oxidation state to a -2 oxidation state in water.
To determine the number of electrons transferred, subtract the oxidation state of iron in the reactants from the oxidation state of iron in the products:
(+3) - (+2) = 1
Therefore, a total of 1 electron is transferred during this reaction.
Hence, in the reaction of hydrogen peroxide with iron (II) ion in acidic solution to form iron (III) ion and water, 1 electron is transferred.