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:

The reaction between zinc and iron sulphate to give zinc sulphate as a product is a _____

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:

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: $\mathrm{Zn}, \mathrm{Cu}, \mathrm{K}, \mathrm{Al}, \mathrm{Hg}, \mathrm{Na}, \mathrm{Ni}, \mathrm{Ag}, \mathrm{Au}$.

Which of the following conditions will increase the voltage of the cell represented by the equation below?

${\mathrm{Cu}}_{\left(\mathrm{s}\right)}+2{\mathrm{Ag}}_{\left(\mathrm{aq}\right)}^{+}⟶{\mathrm{Cu}}_{\left(\mathrm{aq}\right)}^{2+}+2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

Which group of nonmetals is the most reactive?

The tendency of the electrodes made up of $\mathrm{Cu}, \mathrm{Zn}$ and $\mathrm{Ag}$ to release electrons when dipped in their respective salt solutions decreases in the order:

Which process occurs in the electrolysis of an aqueous tin($\mathrm{ll}$) chloride solution at a tin anode?

Select the correct option, for the given standard ${\mathrm{E}}^{\mathrm{o}}$ values of few redox couples:
$\mathrm{Z}{\mathrm{n}}^{2+}/\mathrm{Z}\mathrm{n}=-0.76\mathrm{V}, \mathrm{A}{\mathrm{g}}^{+}/\mathrm{A}\mathrm{g}=+0.80\mathrm{V}, {\mathrm{Cu}}^{2+}/\mathrm{Cu}=0.34\mathrm{V}$
 

Mark the correct statement based on the ${\mathrm{E}}^{\mathrm{o}}$ values of redox couple of halogens given below
$\mathrm{ }{{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{I}}_2/{\mathrm{I}}^{-}}=+0.54\mathrm{V},{{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Br}}_2/{\mathrm{Br}}^{-}}=+1.08\mathrm{V};{{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}}=+1.36\mathrm{V}$.