Electrochemical Series and its Applications

For the reduction of $N{O}_3^{-}$ ion in an aqueous solution, $E°$ is $+0.96V$. Values $E°$ for some metal ions are given below

$\begin{array}{l}{V}^{2+}(aq)+2e^{-}\to VE°=-1.19V\\ F{e}^{3+}(aq)+3e^{-}\to FeE°=-0.04V\\ A{u}^{3+}(aq)+3e^{-}\to AuE°=+1.40V\\ H{g}^{2+}(aq)+2e^{-}\to HgE°=+0.86V\end{array}$

The pair(s) of metals that is (are) oxidized by ${\mathrm{NO}}_3^{-}$ in aqueous solution is/are

The standard reduction potential values of three metallic cations, X, Y and Z are $0.52,-3.03 \mathrm{and}-1.18\mathrm{V}$ respectively. The order of reducing power of the corresponding metals is:

Using the data given below find out the strongest reducing agent?

${\mathrm{E}}_{{\mathrm{C}}_2{\mathrm{O}}_7{}^{2-}/{\mathrm{Cr}}^{3+}}^0=1.33 \mathrm{V} {\mathrm{E}}_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}=1.36 \mathrm{V}}^0$

${\mathrm{E}}_{{\mathrm{MnO}}_4^{-}/{\mathrm{Mn}}^{2+}}^0=1.51 \mathrm{V} {\mathrm{E}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}^0=-0.74 \mathrm{V}$

On the basis of the given following electrode potential, which one is the strongest reducing agent?

${\mathrm{E}}_{{\mathrm{Cr}}_2{\mathrm{O}}_7^{-2}\mid {\mathrm{Cr}}^{3+}}^{°}=1.33 \mathrm{V}$

${{\mathrm{E}}^{°}}_{{\mathrm{MnO}}_4^{-}|{\mathrm{Mn}}^{2+}}=1.51 \mathrm{V}$

${\mathrm{E}}_{{\mathrm{Br}}_2\mid {\mathrm{Br}}^{-}}^{°}=1.09 \mathrm{V}$

${{\mathrm{E}}^{°}}_{{\mathrm{Zn}}^{2+}\mid \mathrm{Zn}}=-0.76 \mathrm{V}$

The standard electrode potentials $\left({\text{E}}_{{\text{M}}^{+}/\text{M}}^{\text{o}}\right)$ of four metals $\text{A,}\text{B,}\text{C}$ and $\text{D}$ are $-\text{1}\text{.2}\text{V,}$$\text{0}\text{.6}\text{V}$, $\text{0}\text{.85}\text{V}$ and $-\text{0}\text{.76}\text{V}$, respectively. The sequence of deposition of metals on applying potential is:

Given:
$\mathrm{C}{\mathrm{o}}^{3+}+{\mathrm{e}}^{-}\to \mathrm{C}{\mathrm{o}}^{2+};\mathrm{E}°=+1.81\mathrm{V}$
${\mathrm{P}\mathrm{b}}^{3+}+{2\mathrm{e}}^{-}\to {\mathrm{P}\mathrm{b}}^{2+};\mathrm{E}°=+1.67\mathrm{V}$
$\mathrm{C}{\mathrm{e}}^{4+}+{\mathrm{e}}^{-}\to \mathrm{C}{\mathrm{e}}^{3+};\mathrm{E}°=+1.61\mathrm{V}$
${\mathrm{B}\mathrm{i}}^{3+}+{3\mathrm{e}}^{-}\to \mathrm{B}\mathrm{i};\mathrm{E}°=+0.20\mathrm{V}$
Oxidizing power of the species will increase in the order:

How many elements among given form dihydrogen on reaction with $\mathrm{HCl}$ :
$\mathrm{Cu},\mathrm{Na},\mathrm{K},\mathrm{Ag},\mathrm{Au},\mathrm{Zn},\mathrm{Ca},\mathrm{Mg}$

Upon dipping a copper rod, the aqueous solution of the salt that can turn blue is:

The pair of metals which will produce hydrogen gas in reaction with acid is:

Which of the following is not an application of electrochemical series?

Consider the following half reactions and choose the correct alternative

${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}⟶2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$ ${\mathrm{E}}^0=1.36\mathrm{V}$

$\begin{array}{ll}{\mathrm{Br}}_2\left(\mathrm{l}\right)+2{\mathrm{e}}^{-}⟶2\mathrm{Br}\left(\text{ aq }\right)& {\mathrm{E}}^0=1.07\mathrm{V}\\ {\mathrm{I}}_2\left(\mathrm{s}\right)+2{\mathrm{e}}^{-}⟶2{\mathrm{I}}^{-}\left(\mathrm{aq}\right)& {\mathrm{E}}^0=0.53\mathrm{V}\end{array}$

The strongest oxidising agent among the species ${In}^{3+}\left({\mathrm{E}}^0=-1.34 \mathrm{V}\right), {\mathrm{Au}}^{3+}\left({\mathrm{E}}^0=1.4 \mathrm{V}\right),{\mathrm{Hg}}^{2+}$$({\mathrm{E}}^0=0.86\mathrm{V}), {\mathrm{Cr}}^{3+}\left({\mathrm{E}}^0=-0.74 \mathrm{V}\right)$ is

The number of metals which can liberate ${\mathrm{H}}_2$ from dilute $\mathrm{HCl}$ is: $\mathrm{Zn}, \mathrm{Cu}, \mathrm{K}, \mathrm{Al}, \mathrm{Hg}, \mathrm{Na}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}$.

In the electrochemical cell : $\mathrm{Zn}\left|{\mathrm{ZnSO}}_4(0.01\mathrm{M})\right| \left|{\mathrm{CuSO}}_4(1.0\mathrm{M})\right|\mathrm{Cu}$, the emf of this Daniel cell is ${\mathrm{E}}_1$. When the concentration of ${\mathrm{ZnSO}}_4$ is changed to $1.0\mathrm{M}$ and that of ${\mathrm{CuSO}}_4$ changed to $0.01\mathrm{M}$, the emf changes to ${\mathrm{E}}_2$. From the followings, which one is the relationship between ${\mathrm{E}}_1$ and ${\mathrm{E}}_2?$ (Given,$\left.\frac{\mathrm{RT}}{\mathrm{F}}=0.059\right)$

What will occur if a block of copper metal is dropped into a beaker containing a solution of $1{\mathrm{MZnSO}}_4$?

Standard electrode potentials of three metals $\mathrm{x},\mathrm{y},\mathrm{z}$ are $0.52 \mathrm{V},-2.87 \mathrm{V}$ and $– 0.44 \mathrm{V}$ respectively. The reducing power of these metals are :

Consider the reaction, ${\mathrm{Mn}}^{{\mathrm{n}}^{+}}(\mathrm{aq}.)+\mathrm{ne}\to {\mathrm{M}}^0( \mathrm{s})$ The standard reduction potential values of the metals ${\mathrm{M}}_{1,}{\mathrm{M}}_2$ and ${\mathrm{M}}_3$ are $-0.34 \mathrm{V},-3.05 \mathrm{V}$ and $-1.66 \mathrm{V}$ respectively. The order of their reducing power will be :

Given:
${{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}=+0.80\mathrm{V}, {\mathrm{E}}_{{\mathrm{Co}}^{2+}/\mathrm{Co}}^{\circ }=-0.28\mathrm{V}$
${{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}=+0.34\mathrm{V}, {{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}=-0.76\mathrm{V}$
Which metal will corrode fastest?