Using Pt

[Haley Dveirin 1E]

When is it necessary to use Pt(s) in the skeletal equation of a redox reaction?

[Sartaj Bal 1J]

Some half reactions have no conducting solids so it is necessary to use an inert conductor (platinum for example) as an electrode to transfer electrons. For the reaction, 2Fe3+ + Cu yields Cu2+ + 2Fe2+, platinum (s) is part of the cathode.

[Nicholas_Gladkov_2J]

When is it necessary to use Pt(s) in the skeletal equation of a redox reaction?

In the example that Dr. Lavelle gave in class: 2Fe3+(aq) + Cu(s) -> Cu2+(aq) + 2Fe2+ although platinum is part of the redox reaction, platinum is an inert conductor that is transferring e-, as there is no conducting solid in the reaction in both reactants and products of the solution. Platinum itself is not loosing or gaining e-, so I'm guessing no.

[Lizette Noriega 1H]

You can use Pt (s) if there is an absence of a solid in a redox reaction; because it is an inert conductor, it will allow for the transfer of electrons without interfering with the reaction itself

[Charlene Datu 2E]

This is a follow-up question about this concept.
Are there other inert conductors that could be used? For example, in the homework for 6L.3B, C(gr) is used as a conductor. Is this an inert conductor because it's in its most stable form?

[WesleyWu_1C]

Lavelle told us in class that Pt and C(gr) are both good inert conductors, but that Pt is more commonly used.

[Kayla Maldonado 1C]

When is it necessary to use Pt(s) in the skeletal equation of a redox reaction?

In the example that Dr. Lavelle gave in class: 2Fe3+(aq) + Cu(s) -> Cu2+(aq) + 2Fe2+ although platinum is part of the redox reaction, platinum is an inert conductor that is transferring e-, as there is no conducting solid in the reaction in both reactants and products of the solution. Platinum itself is not loosing or gaining e-, so I'm guessing no.

Why do we need Pt(s) as the conducting solid if we have Cu(s) in the reaction? Is this solid not a conductor?

[Sarah Zhari 1D]

When is it necessary to use Pt(s) in the skeletal equation of a redox reaction?

In the example that Dr. Lavelle gave in class: 2Fe3+(aq) + Cu(s) -> Cu2+(aq) + 2Fe2+ although platinum is part of the redox reaction, platinum is an inert conductor that is transferring e-, as there is no conducting solid in the reaction in both reactants and products of the solution. Platinum itself is not loosing or gaining e-, so I'm guessing no.

Why do we need Pt(s) as the conducting solid if we have Cu(s) in the reaction? Is this solid not a conductor?

Pt(s) is used to transfer electrons from the Fe3+ (aq) to the copper part of the reaction. The platinum electrode is needed as Fe3+ is in solution.