Question

Identify the species that is oxidized and the species that is reduced in the reaction. Write out half reactions to show how many electrons are gained or lost by each species. Include the state of each species in the equation. Fe3+(aq) + Al(s) ? Al3+(aq) + Fe(s) Fe3+ reduced , Al oxidized Oxidation Reaction: Reduction Reaction:

          Identify the species that is oxidized and the species that is reduced in the reaction. Write out half
reactions to show how many electrons are gained or lost by each species. Include the state of each
species in the equation.

Fe3+(aq) + Al(s) ? Al3+(aq) + Fe(s)

Fe3+ reduced , Al oxidized

Oxidation Reaction:
Reduction Reaction:

Identify the species that is oxidized and the species that is reduced in the reaction. Write out half
reactions to show how many electrons are gained or lost by each species. Include the state of each
species in the equation.

Fe3+(aq) + Al(s) ? Al3+(aq) + Fe(s)

Fe3+ reduced , Al oxidized

Oxidation Reaction:
Reduction Reaction:

Added by John W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Nicole Krahulik

07/14/2023

Step 1

Fe(II) (aq) + Al (s) -> Al(III) (aq) + Fe (s) Now, we can see the changes in oxidation states: Fe(II) (aq) -> Fe (s) : Fe goes from +2 to 0, so it gains 2 electrons (reduction) Al (s) -> Al(III) (aq) : Al goes from 0 to +3, so it loses 3 electrons (oxidation) Show more…

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Identify the species that is oxidized and the species that is reduced in the reaction. Write out half reactions to show how many electrons are gained or lost by each species. Include the state of each species in the equation. Fe(s) + Al3+(aq) -> Al(s) + Fe2+(aq) Oxidized: Fe(s) Reduced: Al3+(aq) Oxidation Reaction: Fe(s) -> Fe2+(aq) + 2e- Reduction Reaction: Al3+(aq) + 3e- -> Al(s)