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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.
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?
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.
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?
