Calculate the standard cell potential (in V) | vedclass

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(D) The cell reaction is: $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} 	o Fe^{3+}_{(aq)} + Ag_{(s)}$Given standard reduction potentials:$(1)$ $Ag^{+} + e^{-} 	o

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$x + 2y - 3z$

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(D) The cell reaction is: $Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} 	o Fe^{3+}_{(aq)} + Ag_{(s)}$Given standard reduction potentials:$(1)$ $Ag^{+} + e^{-} 	o Ag$,$E^o = x \ V$,$\Delta G^o_1 = -nFE^o = -1 \cdot F \cdot x = -Fx$$(2)$ $Fe^{2+} + 2e^{-} 	o Fe$,$E^o = y \ V$,$\Delta G^o_2 = -2Fy$$(3)$ $Fe^{3+} + 3e^{-} 	o Fe$,$E^o = z \ V$,$\Delta G^o_3 = -3Fz$We need to find the $\Delta G^o$ for the reaction: $Fe^{2+} 	o Fe^{3+} + e^{-}$This can be obtained by: (Reaction $2$) - (Reaction $3$)$\Delta G^o_{oxidation} = \Delta G^o_2 - \Delta G^o_3 = -2Fy - (-3Fz) = 3Fz - 2Fy$For the total cell reaction:$Fe^{2+} + Ag^{+} 	o Fe^{3+} + Ag$$\Delta G^o_{cell} = \Delta G^o_{oxidation} + \Delta G^o_1 = (3Fz - 2Fy) + (-Fx) = -F(x + 2y - 3z)$Since $\Delta G^o_{cell} = -nFE^o_{cell}$ and $n = 1$:$-FE^o_{cell} = -F(x + 2y - 3z)$$E^o_{cell} = x + 2y - 3z \ V$

Calculate the standard cell potential (in $V$) of the cell in which the following reaction takes place:
$Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \to Fe^{3+}_{(aq)} + Ag_{(s)}$
Given that:
$E^o_{Ag^{+}/Ag} = x \ V$
$E^o_{Fe^{2+}/Fe} = y \ V$
$E^o_{Fe^{3+}/Fe} = z \ V$

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Calculate the standard cell potential (in $V$) of the cell in which the following reaction takes place:$Fe^{2+}_{(aq)} + Ag^{+}_{(aq)} \to Fe^{3+}_{(aq)} + Ag_{(s)}$Given that:$E^o_{Ag^{+}/Ag} = x \ V$$E^o_{Fe^{2+}/Fe} = y \ V$$E^o_{Fe^{3+}/Fe} = z \ V$