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 –

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

Which of the following choices of $\mathrm{X}$ and $\mathrm{Y}$ would make the reaction

$\mathrm{X}\left(\mathrm{s}\right)+{\mathrm{Y}}^{2+}\left(\mathrm{aq}\right)\to {\mathrm{X}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Y}\left(\mathrm{s}\right)$ spontaneous at $298 \mathrm{K}$?

[at $298 \mathrm{K}$, use standard reduction potentials: ${\mathrm{E}}^0\left({\mathrm{Zn}}^{2+}/\mathrm{Zn}\right)=-0.76 \mathrm{V};{\mathrm{E}}^0\left({\mathrm{Ni}}^{2+}/\mathrm{Ni}\right)=-0.23 \mathrm{V}$;$\mathrm{E}°\left({\mathrm{Fe}}^{2+}/\mathrm{Fe}\right)=-0.44 \mathrm{V}$]

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

A solution is 1 molar in each of $\mathrm{NaCl}, {\mathrm{CdCl}}_2, {\mathrm{ZnCl}}_2$ and ${\mathrm{PbCl}}_2$. To this $\mathrm{Sn}$ metal is added, which of the following is true?
Given $\mathrm{E}°\left({\mathrm{Pb}}^{2+}/\mathrm{Pb}=-0.126 \mathrm{V}\right)$

${\mathrm{E}}_{\mathrm{Sn}°/\mathrm{Sn}}^{°}=-0.136 \mathrm{V}, {\mathrm{E}}_{\mathrm{Cd}°/\mathrm{Cd}}^{°}=-0.40 \mathrm{V}$

${\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^{°}=-0.763 \mathrm{V}, {\mathrm{E}}_{{\mathrm{Na}}^{+}/\mathrm{Na}}^{°}=-2.71 \mathrm{V}$

For a galvanic cell $\mathrm{Cr}/{\mathrm{Cr}}^{3+}//{\mathrm{cd}}^2/\mathrm{Cd}$$,$ calculated ${\mathrm{\Delta G}}^0$ for its all reaction will be
$\left[{\mathrm{E}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^0=-0.74\mathrm{V},{\mathrm{E}}_{{\mathrm{Cd}}^{2+}/\mathrm{Cd}}^0=-0.40 \mathrm{V}\right]$

Given half-cell potentials ${\mathrm{E}}_{{\mathrm{Cr}}^{3+}/{\mathrm{Cr}}^{2+}}^{0^{2+}}=-0.4 \mathrm{V}$ and ${\mathrm{E}}_{{\mathrm{Cr}}^{2+}/\mathrm{cr}}^0=-0.91 \mathrm{V}$, find the standard reduction potential of ${\mathrm{Cr}}^{3+}/\mathrm{Cr}$

The standard reduction potential for $Z{n}^{2+}/Zn, N{i}^{2+}/N\mathrm{i }\mathrm{a}\mathrm{n}\mathrm{d}\mathrm{ }F{e}^{2+}/Fe$ are respectively $-0.76, -0.23 \mathrm{a}\mathrm{n}\mathrm{d}-0.44\mathrm{ }\mathrm{V}$ . The reaction $X+Y^{2+}\to X^{2+}+Y$ will have more negative $\mathrm{\Delta }G$ value when $X$ and $Y$ are-