Electrode Potential and Standard Electrode Potential

A standard hydrogen electrode has zero electrode potential because

When the samples of copper with zinc impurity is to be purified by electrolysis, the appropriate electrodes are –

Which of the following is oxidised by oxygen in acidic medium?

Which of the following facts is not true?

Consider the following four electrodes:

$\mathrm{P}: {\mathrm{Cu}}^{2+}\left(0.0001 \mathrm{M}\right)/\mathrm{Cu}\left(\mathrm{s}\right)$, $\mathrm{Q}: {\mathrm{Cu}}^{2+}\left(0.1 \mathrm{M}\right)/\mathrm{Cu}\left(\mathrm{s}\right)$, $\mathrm{R}: {\mathrm{Cu}}^{2+}\left(0.01 \mathrm{M}\right)/\mathrm{Cu}\left(\mathrm{s}\right)$ and $\mathrm{S}: {\mathrm{Cu}}^{2+}\left(0.001 \mathrm{M}\right)/\mathrm{Cu}\left(\mathrm{s}\right)$

If the standard electrode potential of ${\mathrm{Cu}}^{2+}/\mathrm{Cu}$ is $+0.34 \mathrm{V}$, the reduction potentials in volts of the above electrodes follow the order:

Electrode potential of any electrode depends on 

In the transition metal $3\mathrm{d}$ series, the positive ${\mathrm{M}}^{2+}/\mathrm{M}$ standard electrode potential is shown by

The reaction $\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)\to {\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Cu}\left(\mathrm{s}\right)$ at $300 \mathrm{K}$ has$E_{cell}^0=1.2 \mathrm{V}.$ The equilibrium constant for this reaction is $(2.303 \mathrm{R} \mathrm{T} / \mathrm{F}=0.06 \mathrm{V})$

The value of potential of the cell in which the following reaction takes place at $298 \mathrm{K}$ is

[At $298 \mathrm{K},{\mathrm{E}}^0\left({\mathrm{Ag}}^{+}/\mathrm{Ag}\right)=+0.80 \mathrm{V};{\mathrm{E}}^0\left({\mathrm{Al}}^{3+}/\mathrm{Al}\right)=-1.66 \mathrm{V};2.303\mathrm{RT}/\mathrm{F}=0.06 \mathrm{V}$ ]

$\mathrm{Al}\left(\mathrm{s}\right)+3{\mathrm{Ag}}^{+}(0.001\mathrm{M})\to {\mathrm{Al}}^{3+}(0.1\mathrm{M})+3\mathrm{Ag}\left(\mathrm{s}\right)$

Standard electrode potentials of redox couples ${\mathrm{A}}^{2+}/\mathrm{A}, {\mathrm{B}}^{2+}/\mathrm{B}, \mathrm{C}/{\mathrm{C}}^{2+}$ and ${\mathrm{D}}^{2+}/\mathrm{D}$ are $0.3 \mathrm{V},-0.5 \mathrm{V},-0.75 \mathrm{V}$ and $0.9 \mathrm{V}$ respectively. Which of these is best oxidising agent and reducing agent respectively?

Three metals $\mathrm{A},\mathrm{B}$, and $\mathrm{C}$ are arranged in increasing order of standard reduction electrode potential, hence their chemical reactivity order will

$\frac{1}{2}{\mathrm{F}}_2+{\mathrm{e}}^{-}\to {\mathrm{F}}^{-} {\mathrm{E}}^{\mathrm{o}}=+3.02\mathrm{V}$

Electrode potential for given reaction

${\mathrm{F}}_2+2{\mathrm{e}}^{-}\to 2{\mathrm{F}}^{-}$

Standard reduction potential is calculated at

Select the correct statement.

Given that ${{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}=0.80 \mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Mg}}^{2+}/\mathrm{Mg}}=-2.37 \mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}=0.34 \mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Hg}}^{2+}/\mathrm{Hg}}=0.79 \mathrm{V}$.

The standard reduction potentials at $25°\mathrm{C}$ of ${\mathrm{Li}}^{+}/\mathrm{Li}$,${\mathrm{Ba}}^{2+}/\mathrm{Ba}$, ${\mathrm{Na}}^{+}/\mathrm{Na}$ and ${\mathrm{Mg}}^{2+}/\mathrm{Mg}$ are $-\mathrm{a}$, $\left(-\mathrm{a}+0.15\right),\left(-\mathrm{a}+0.34\right)$ and $\left(-\mathrm{a}+0.68\right)$ volt respectively. The strongest oxidising agent among the following is

Metal which will easily release electron (s) in aqueous solution, is

The electode potential of anode at standard condition is called standard _____ potential.

The standard oxidation potential of zinc is _____ .