Electrochemical Series and its Applications

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 position of some metals in the electrochemical series in decreasing electropositive character is$\mathrm{Mg}>\mathrm{Al}>$$\mathrm{Zn}>\mathrm{Cu}>\mathrm{Ag}.$ The change expected on stirring the solution of aluminium nitrate with copper spoon is

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

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

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:

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
$\mathrm{ }{{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{I}}_2/{\mathrm{I}}^{-}}=+0.54\mathrm{V},{{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Br}}_2/{\mathrm{Br}}^{-}}=+1.08\mathrm{V};{{\mathrm{E}}^{\mathrm{o}}}_{{\mathrm{Cl}}_2/{\mathrm{Cl}}^{-}}=+1.36\mathrm{V}$.

Which element can reduce Aluminium?

Among the following, which is the most reactive metal which displaces other metals from their salts in solution?

${\mathrm{E}}_{\mathrm{Z}\mathrm{n}/\mathrm{Z}{\mathrm{n}}^{2+}}^0=+0.76\mathrm{V},\mathrm{ }{\mathrm{E}}_{\mathrm{A}\mathrm{g}/\mathrm{A}{\mathrm{g}}^{+}}^0=-0.80\mathrm{V},\mathrm{ }$

${\mathrm{E}}_{\mathrm{C}\mathrm{u}/\mathrm{C}{\mathrm{u}}^{2+}}^0=-0.34\mathrm{V},\mathrm{ }{\mathrm{E}}_{\mathrm{C}\mathrm{o}/\mathrm{C}{\mathrm{o}}^{+2}}^0=0.28\mathrm{V}$

${\mathrm{F}}_2$ can easily oxidise which of the following?

We have taken two electrode, with potential values: ${\mathrm{E}}_{{\mathrm{Mg}}^{2+}/\mathrm{Mg}}^{\mathrm{a}}=- 2.37 \mathrm{V} \mathrm{and} {{\mathrm{E}}^{\mathrm{b}}}_{{\mathrm{Fe}}^{3+}/\mathrm{Fe} }=-0.04 \mathrm{V}$. Which of the following will act as the best reducing agent:

Given electrode potentials: 

$$\begin{gathered} {\mathrm{Ag}}^{+}/\mathrm{Ag}=+0.80 \mathrm{V} , {\mathrm{Co}}^{2+}/\mathrm{Co}=-0.28 \mathrm{V} \\ {\mathrm{Cu}}^{2+}/\mathrm{Cu}=+0.34 \mathrm{V}, {\mathrm{Zn}}^{2+}/\mathrm{Zn}=-0.76 \mathrm{V} \end{gathered}$$

Among these four metals, which can displace all other metals from their salts in a solution?