Electrochemical Series

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 number of correct statements from the following is...........
A. ${\mathrm{E}}_{\mathrm{cell}}$ is an intensive parameter
B. A negative ${\mathrm{E}}^{\mathrm{o}}$ means that the redox couple is a stronger reducing agent than the ${\mathrm{H}}^{+}/{\mathrm{H}}_2$ couple.
C. The amount of electricity required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
D. The amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolyte.

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?

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

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

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

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

Predict reaction of 1 N sulphuric acid with Copper. Given, ${\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{°}=+0.34 \mathrm{V}$.

Higher is the reduction potential of non-metals, higher is the reactivity.

Higher is the reduction potential of non-metals, higher is the reactivity.

${\mathrm{H}}_2$ cannot be displaced by

The standard electrode potential of ${\mathrm{M}}^{2+}/\mathrm{M}$ is positive for

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

Higher reduction potential increases the reactivity of non-metals.

What is the affect of reduction potential on the reactivity of non-metals?

Which halogen will be more reactive?

Reduction potential of bromine- $+1.07\mathrm{V}$ or reduction potential of chlorine- $1.36\mathrm{V}$.

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: