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?

2e + 2H^+ + H2O2==> 2H2O is one half reaction.

Fe^+2 ==> Fe^+3 + 1e is the other.

To determine how many electrons are transferred in the reaction of hydrogen peroxide with iron (II) ion in acidic solution, you need to examine the balanced redox equation for the reaction. Let's start by writing the balanced equation for the reaction:

H2O2 + Fe2+ → Fe3+ + H2O

In acidic solution, H+ ions are present on both sides of the reaction. The next step is to balance the equation by adding H2O and H+ ions as needed. The balanced equation is as follows:

H2O2 + 2 H+ + 2 Fe2+ → 2 Fe3+ + 2 H2O

Now, we need to identify the atoms that undergo oxidation and reduction. In this reaction, iron (II) ions (Fe2+) are oxidized to iron (III) ions (Fe3+), and hydrogen peroxide (H2O2) is reduced to water (H2O).

Since the iron ions are gaining an electron during oxidation, we need to multiply their coefficient by the number of electrons gained during the reaction. In this case, each iron (II) ion (Fe2+) gains one electron, so the total number of electrons transferred is equal to the coefficient of Fe2+ (which is 2) multiplied by the number of Fe2+ ions involved in the reaction (which is 2). Therefore, a total of 4 electrons are transferred.

To summarize, in the reaction of hydrogen peroxide with iron (II) ion in acidic solution to form iron (III) ion and water, 4 electrons are transferred.