The two half-cell reactions of an electrochemical cell is given as Ag + + e − ⟶ Ag ; E Ax + / Ag ∘ = − 0.3995 V Fe 3 + ⟶ Fe 3 ∗ + e − ; E Fe 3 + Fv 2 + = − 0.7120 V . The value of cell E

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The two ​ half-cell ​ reactions ​ of ​ an ​ electrochemical cell is given as Ag + + e − ⟶ Ag ; E Ax + / Ag ∘ ​ = − 0.3995 V Fe 3 + ⟶ Fe 3 ∗ + e − ; E Fe 3 + Fv 2 + ​ = − 0.7120 V . The value of cell EMF will be

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Species with more negative E ∘ (standard reduction potential) generally acts as reducing agent while with less negative E ∘ acts as oxidising agent. Thus, the overall reaction is Ag + + Fe 2 + Δ E ∘ ​ ⟶ Fe 3 + + Ag = E OA ∘ ​ − E RA ∘ ​ = − 0.3995 − ( − 0.7120 ) V = − 0.3995 + 0.7120 V = + 0.3125 V ​

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