Electrodes and Electrode Potentials

A standard hydrogen electrode has zero electrode potential because

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:

Define standard oxidation electrode potential.

Define electrode.

In a voltaic cell, reduction occurs at cathode

In an electrochemical cell, reduction occurs at anode.

The negative terminal of electrochemical cell is

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 hydrogen electrode is the reference electrode.

Explain standard hydrogen electrode.

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

Electrode potential for given reaction

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

Standard reduction potential is calculated at

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 gas liberated at the cathode is
 

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 ${\mathrm{Cr}}^{3+}/\mathrm{Cr}$