The standard reduction potential for Fe^{2+}/ | vedclass

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(D) The given cell reaction is: $Fe^{2+} + Sn \longrightarrow Fe + Sn^{2+}$In this reaction,$Fe^{2+}$ is reduced to $Fe$ (cathode) and $Sn$ is oxidize

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$-0.30 \ V$

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(D) The given cell reaction is: $Fe^{2+} + Sn \longrightarrow Fe + Sn^{2+}$In this reaction,$Fe^{2+}$ is reduced to $Fe$ (cathode) and $Sn$ is oxidized to $Sn^{2+}$ (anode).The standard reduction potentials are given as: $E^o_{Fe^{2+}/Fe} = -0.44 \ V$ and $E^o_{Sn^{2+}/Sn} = -0.14 \ V$.The standard emf of the cell $(E^o_{cell})$ is calculated as:$E^o_{cell} = E^o_{cathode} - E^o_{anode}$$E^o_{cell} = E^o_{Fe^{2+}/Fe} - E^o_{Sn^{2+}/Sn}$$E^o_{cell} = -0.44 \ V - (-0.14 \ V)$$E^o_{cell} = -0.44 + 0.14 = -0.30 \ V$

The standard reduction potential for $Fe^{2+}/Fe$ and $Sn^{2+}/Sn$ electrodes are $-0.44 \ V$ and $-0.14 \ V$ respectively. For the cell reaction,$Fe^{2+} + Sn \longrightarrow Fe + Sn^{2+}$,the standard emf is:

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