Complete the following ionic equation for this reaction.
2Fe^2+ + H2O2 + 2H^+
2Fe^3+ + 2H2O
Does the Fe^2+ undergo oxidation or reduction?
The Fe^2+ undergoes oxidation.
Write half equation
Fe^2+ -> Fe^3+ + e^-
The given reaction is:
2Fe^2+ + H2O2 + 2H^+ → ?
To complete the ionic equation, we need to consider the chemical species in the reaction and determine their respective ionic forms, including any changes in oxidation states.
First, let's identify the oxidation states of each element in the reactants:
- Fe: The Fe ion (Fe^2+) has an oxidation state of +2.
- H: Hydrogen exists as H^+ in an acidic solution, indicating an oxidation state of +1.
- O: Oxygen typically has an oxidation state of -2, so for H2O2, each hydrogen has an oxidation state of +1, and each oxygen has an oxidation state of -1.
Now, let's balance the equation by ensuring that the number of atoms and charges are equal on both sides.
After balancing, the complete ionic equation is:
2Fe^2+ + H2O2 + 4H^+ → 2Fe^3+ + 2H2O
Therefore, the balanced and completed ionic equation for this reaction is:
2Fe^2+ + H2O2 + 4H^+ → 2Fe^3+ + 2H2O.
To complete the ionic equation for this reaction, we need to determine the products that are formed when 2Fe^2+, H2O2, and 2H^+ react.
Let's break down the reactants and identify their ionic forms:
2Fe^2+ - This represents two ions of iron with a charge of +2.
H2O2 - This represents hydrogen peroxide, which can dissociate into two H+ ions and one O2^2- ion.
2H^+ - This represents two hydrogen ions with a charge of +1 each.
Now, let's find the products of this reaction:
The hydrogen ions (H+) react with the hydrogen peroxide (H2O2) to form water (H2O):
2H^+ + H2O2 -> 2H2O
The two Fe^2+ ions remain unchanged and are not involved in the reaction.
Therefore, the complete ionic equation for this reaction is:
2Fe^2+ + H2O2 + 2H^+ -> 2Fe^2+ + 2H2O