Understanding Voltaic Cells: The Role of Fe3+ in the Anode

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In a voltaic cell, the presence of Fe3+ in the anode solution is essential for maintaining the standard conditions of 1.0 mol/L concentration at SATP. Although Fe3+ is a product of the oxidation reaction, its initial presence ensures that the half-cell reaction can proceed effectively. The inclusion of reaction products in the anode helps maintain equilibrium and allows for continuous electron flow. This setup is crucial for the proper functioning of all voltaic cells, as it aligns with the definition of standard conditions. Understanding this role clarifies the necessity of having products present initially in the anode.
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The problem I have is just a detail I want to clarify about the voltaic cell.

A standard cell is a voltaic cell in which each half-cell contains all entities shown in the half-reaction equation at SATP conditions, with a concentration of 1.0 mol/L for the aqueous solution.

vcrqc4.jpg


Referring to the both the definition and the diagram, what I'm wondering is: why is it necessary to have the Fe 3+ (aq) in the anode solution? It's the product of the oxidation reaction occurring there, so why is it neededthere initially ? This includes not only the particular cell shown above, but all voltaic cells. In general, why is it necessary to have the product of the half-reaction in the anode half? What function does it serve in the cell?
 
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Generally speaking - there is no need for products to be present initially. They will appear immediately given chance :wink:

However, at STP - by definition - activity of every reagent involved is 1.
 

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