In FeO(aq) + V2O5(aq) → Fe2O3(aq) + VO(aq), which species acts as the reducing agent?

Prepare for the Electrochemistry Test with our extensive quiz. Utilize flashcards and multiple-choice questions with detailed hints and explanations to excel in your exam!

Multiple Choice

In FeO(aq) + V2O5(aq) → Fe2O3(aq) + VO(aq), which species acts as the reducing agent?

Explanation:
In redox reactions, the reducing agent is the species that donates electrons and gets oxidized. Look at oxidation states: FeO has iron in the +2 state, while Fe2O3 has iron in the +3 state. Fe is losing electrons as it goes from +2 to +3, so FeO is the source of electrons and is oxidized. That makes FeO the reducing agent. The vanadium species tell the opposite story: V2O5 has vanadium at +5, and VO has vanadium at +2, so vanadium is gaining electrons (being reduced) and V2O5 is the oxidizing agent. So FeO donates the electrons and acts as the reducing agent.

In redox reactions, the reducing agent is the species that donates electrons and gets oxidized.

Look at oxidation states: FeO has iron in the +2 state, while Fe2O3 has iron in the +3 state. Fe is losing electrons as it goes from +2 to +3, so FeO is the source of electrons and is oxidized. That makes FeO the reducing agent.

The vanadium species tell the opposite story: V2O5 has vanadium at +5, and VO has vanadium at +2, so vanadium is gaining electrons (being reduced) and V2O5 is the oxidizing agent.

So FeO donates the electrons and acts as the reducing agent.

More Multiple Choice Questions
Subscribe

Get the latest from Passetra

You can unsubscribe at any time. Read our privacy policy