Half/Rxn & Balanced Equations for galvanic cells.
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Half/Rxn & Balanced Equations for galvanic cells.
In homework problem 6L3, Platinum appears on both the cathode and anode side of the diagram. I was wondering what this means exactly, and what needs to be done depending on which side it's on?
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Re: Half/Rxn & Balanced Equations for galvanic cells.
It just implies that none of your species are solids. They’re either (aq) or (g) if you’re talking about example d
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Re: Half/Rxn & Balanced Equations for galvanic cells.
Pt(s) is added to either the anode or cathode (or even both) when there is no solid metal conductor present.
Re: Half/Rxn & Balanced Equations for galvanic cells.
Does anyone know how to write half reactions when reducing and oxidizing agent is the same
Re: Half/Rxn & Balanced Equations for galvanic cells.
we typically add platinum to either (or both) side of the cell diagram if there isn't already an electrode in it
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Re: Half/Rxn & Balanced Equations for galvanic cells.
Mandeep Garcha 2H wrote:Pt(s) is added to either the anode or cathode (or even both) when there is no solid metal conductor present.
Is pt the only metal that we use? at least for the purpose of what we're doing in chem 14B?
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Re: Half/Rxn & Balanced Equations for galvanic cells.
Cells typically need some solid electrode for it to work. So if your equation does not have a solid in it, we have to add Pt(s) at the ends of the cell diagram to show that it is the electrode that passes electrons from the anode to the cathode.
Re: Half/Rxn & Balanced Equations for galvanic cells.
Cells need solids electrodes in both sides to work, so if there is no solid electrode on any side, you place solid platinum to fulfill that necessity.
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Re: Half/Rxn & Balanced Equations for galvanic cells.
Platinum is the most common electrode used in electrochemical cells when none of the species present are solid metals because it is resistant to oxidation and won't easily react in redox reactions.
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