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(B) The cell reaction is $Fe^{2+} + Ag^{+} \rightarrow Fe^{3+} + Ag$.This can be split into two half-reactions:Oxidation: $Fe^{2+} \rightarrow Fe^{3+}

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$x + 2y - 3z$

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(B) The cell reaction is $Fe^{2+} + Ag^{+} \rightarrow Fe^{3+} + Ag$.This can be split into two half-reactions:Oxidation: $Fe^{2+} \rightarrow Fe^{3+} + e^-$Reduction: $Ag^+ + e^- \rightarrow Ag$We are given:$(1)$ $Ag^+ + e^- \rightarrow Ag, \ E^0 = x \ V, \ \Delta G_1^0 = -F(x)$$(2)$ $Fe^{2+} + 2e^- \rightarrow Fe, \ E^0 = y \ V, \ \Delta G_2^0 = -2F(y)$$(3)$ $Fe^{3+} + 3e^- \rightarrow Fe, \ E^0 = z \ V, \ \Delta G_3^0 = -3F(z)$We need the potential for $Fe^{2+} \rightarrow Fe^{3+} + e^-$. Let this be $E^0_{ox}$.Using Hess's Law for $\Delta G^0$:$\Delta G^0(Fe^{2+}$ $\rightarrow Fe^{3+} + e^-) = \Delta G^0(Fe^{2+}$ $\rightarrow Fe) - \Delta G^0(Fe^{3+}$ $\rightarrow Fe)$$-1F(E^0_{ox}) = -2F(y) - (-3F(z))$$-F(E^0_{ox}) = -2Fy + 3Fz$$E^0_{ox} = 2y - 3z$Now,$E^0_{cell} = E^0_{red} + E^0_{ox} = x + (2y - 3z) = x + 2y - 3z$.

For the given cell reaction $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \rightarrow Fe^{3+}_{(aq)} + Ag_{(s)}$,the standard cell potential is:
Given:
$Ag^{+} + e^{-} \rightarrow Ag \quad E^0 = x \ V$
$Fe^{2+} + 2e^{-} \rightarrow Fe \quad E^0 = y \ V$
$Fe^{3+} + 3e^{-} \rightarrow Fe \quad E^0 = z \ V$

Similar Questions

Given,for $Sn^{4+} / Sn^{2+}$,standard reduction potential is $0.15 \ V$ and for $Au^{3+} / Au$,standard reduction potential is $1.5 \ V$. For the reaction,$3 Sn^{2+} + 2 Au^{3+} \longrightarrow 3 Sn^{4+} + 2 Au$,the value of $E_{\text{cell}}^{\circ}$ is:

If the $\Delta G$ of a cell reaction $AgCl + e^- \to Ag + Cl^{-}$ is $-21.20 \ kJ$,the standard e.m.f. of the cell is ............ $V$.

Which among the following species is reduced by tin easily?

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$E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$

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For the given cell reaction $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \rightarrow Fe^{3+}_{(aq)} + Ag_{(s)}$,the standard cell potential is:Given:$Ag^{+} + e^{-} \rightarrow Ag \quad E^0 = x \ V$$Fe^{2+} + 2e^{-} \rightarrow Fe \quad E^0 = y \ V$$Fe^{3+} + 3e^{-} \rightarrow Fe \quad E^0 = z \ V$