Question

Write a balanced equation from the following cell notation: Fe(s) | Fe²+(aq) || NO₃(aq) | NO(g) | Pt(s) include the physical stale of each reactant and product.

Answer 1

To obtain the balanced chemical equation for the given cell notation, separate half-reactions for the anode (oxidation) and cathode (reduction) are written and combined while ensuring electron and charge balance.

Step-by-step explanation:

The student is asking to write a balanced chemical equation from provided cell notation. This notation corresponds to an electrochemical cell setup, and we need to write separate half-reactions for the cathode and the anode and then combine them to get the overall balanced chemical equation.

The cell notation given is: Fe(s) | Fe²+(aq) || NO₃⁻(aq) | NO(g) | Pt(s)

For the oxidation half-reaction at the anode we have:

Fe(s) → Fe²+(aq) + 2e⁻

And for the reduction half-reaction at the cathode we would have something like:

NO₃⁻(aq) + 3e⁻ + 4H+(aq) → NO(g) + 2H₂O(l)

Note that the reduction half-reaction may vary based on the complete cell reaction. Now we combine these half-reactions ensuring the electrons are balanced:

Fe(s) + 4HNO₃(aq) → Fe(NO₃)₃(aq) + NO(g) + 2H₂O(l)

The reaction must also be charge-balanced and may require additional balancing of the HNO₃ and water molecules.