Using the standard electrode potentials given below identify the correct statements from the following. $$…
Using the standard electrode potentials given below identify the correct statements from the following.
$$
\begin{aligned}
\mathrm{Fe}^{2+}+2 e^{-} \longrightarrow \mathrm{Fe} ; E^{\circ} & =-0.44 \mathrm{~V} \\
\mathrm{Cu}^{2+}+2 e^{-} \longrightarrow \mathrm{Cu} ; E^{\circ} & =+0.34 \mathrm{~V} \\
\mathrm{Ag}^{+}+e^{-} \longrightarrow \mathrm{Ag} ; E^{\circ} & =+0.80 \mathrm{~V}
\end{aligned}
$$
(i) Copper can displace iron from $\mathrm{FeSO}_4$ solution.
(ii) Iron can displace copper from $\mathrm{CuSO}_4$ solution.
(iii) Silver can displace copper from $\mathrm{CuSO}_4$ solution.
(iv) Iron can displace silver from $\mathrm{AgNO}_3$ solution.
(i), (ii)
(ii), (iii)
(ii), (iv)
(i), (iv)
Solution
$
\begin{gathered}
\mathrm{Fe}^{2+}+2 e^{-} \longrightarrow \mathrm{Fe} ; E^{\circ}=-0.44 \\
\mathrm{Cu}^{2+}+2 e^{-} \longrightarrow \mathrm{Cu} ; E^{\circ}=+0.34 \\
\mathrm{Ag}+1 e^{-} \longrightarrow \mathrm{Ag} ; E^{\circ}=+0.80
\end{gathered}
$
If a metal have negative electrode potential than metal easily displace, other metal, i.e. Fe can displace $\mathrm{Cu}$ and $\mathrm{Ag}$