1. Tardigrade
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  3. Chemistry
  4. The standard electrode potential for the half-cell reactions are Zn 2++2 e- longrightarrow Zn ; E°=-0.76 V Fe 2++2 e- longrightarrow Fe ; E°=-0.44 V The emf of the cell reaction, Fe 2++ Zn longrightarrow Zn 2++ Fe is

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Q. The standard electrode potential for the half-cell reactions are
$Zn ^{2+}+2 e^{-} \longrightarrow Zn ; E^{\circ}=-0.76 \,V $
$Fe ^{2+}+2 e^{-} \longrightarrow Fe ; E^{\circ}=-0.44 \,V$
The emf of the cell reaction,
$Fe ^{2+}+ Zn \longrightarrow Zn ^{2+}+ Fe$ is

AIPMTAIPMT 1996Electrochemistry

Solution:

$\begin{aligned} E _{\text {cell }}^{0} &=\left( E _{ Fe ^{2+} Fe }^{0}+ E _{ ZnZnh ^{2+}}^{0}\right) \\ &=(-0.44 V +0.76) \\ E ^{0} &=+0.32 V \text { olt } \end{aligned}$