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(D) The standard reduction potentials $(E^{0})$ at $298 \; K$ are as follows:$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}, E^{0} = +1.40 \; V$$Fe^{2+} + 2e^

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$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}$

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(D) The standard reduction potentials $(E^{0})$ at $298 \; K$ are as follows:$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}, E^{0} = +1.40 \; V$$Fe^{2+} + 2e^{-} \rightarrow Fe_{(s)}, E^{0} = -0.44 \; V$$Mg^{2+} + 2e^{-} \rightarrow Mg_{(s)}, E^{0} = -2.36 \; V$$K^{+} + 1e^{-} \rightarrow K_{(s)}, E^{0} = -2.93 \; V$According to the electrochemical series,the species with the highest positive standard reduction potential occupies the top position. Therefore,$Au^{3+} + 3e^{-} \rightarrow Au_{(s)}$ is at the top.

Identify the reaction from the following that occupies the top position in the $EMF$ series (standard reduction potential) at $298 \; K$.

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Addition of powdered lead and iron to a solution which is $1.0 \, M$ in both $Pb^{2+}$ and $Fe^{2+}$ would result in [$E^{\circ}_{Fe^{2+}/Fe} = -0.44 \, V$ and $E^{\circ}_{Pb^{2+}/Pb} = -0.13 \, V$]

What is the decreasing order of deposition of metal on electrode if standard reduction potentials are given as: $Ag^{+} | Ag = 0.80 \ V$,$Cu^{2+} | Cu = 0.337 \ V$,$Sn^{2+} | Sn = -0.136 \ V$,$Cd^{2+} | Cd = -0.403 \ V$?

$2H^{+} \, (aq) + 2e^- \to H_2 \, (g)$. The standard electrode potential for the above reaction is (in volts):

Given:
$E^o_{Fe^{3+} /Fe} = -0.036 \ V, E^o_{Fe^{2+} /Fe} = -0.439 \ V$
The value of standard electrode potential for the change,
$Fe^{3+}_{(aq)} + e^- \rightarrow Fe^{2+}_{(aq)}$ will be ........ $V$.

The standard reduction potentials for $Cu^{2+}|Cu$ and $Cu^{2+}|Cu^{+}$ are $0.337 \, V$ and $0.153 \, V$ respectively. What is the standard electrode potential for the $Cu^{+}|Cu$ half-cell in $V$?

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