Redox Reactions and Electrode Processes

What is the standard electrode potential of hydrogen electrode in volts?

A solution containing one mole per litre each of $\mathrm{AX},{\mathrm{BX}}_2,{\mathrm{CX}}_2$ and ${\mathrm{DX}}_2$ is electrolysed using inert electrodes. The values of the standard potentials for reduction reactions of ${\mathrm{A}}^{+}\mid \mathrm{A},{\mathrm{B}}^{2+}$ $\left|\mathrm{B},{\mathrm{C}}^{2+}\right|\mathrm{C}$ and ${\mathrm{D}}^{2+}\mid \mathrm{Dare}+0.80,+0.34,-0.76$ and $-1.66$ volts respectively. The correct sequence in which these metals will be deposited on the cathode is :

Find ${\mathrm{E}}_{\mathrm{cell}}°$ for the reaction :
$3\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{Cr}}^{+3}(\mathrm{aq}.)\to 3{\mathrm{Zn}}^{+2}(\mathrm{aq}.)+2\mathrm{Cr}\left(\mathrm{s}\right)$
Given : ${\mathrm{E}}_{\left({\mathrm{Zn}}^{+2}/\mathrm{Zn}\right)}^{\mathrm{o}}=-0.76 \mathrm{V}; {\mathrm{E}}_{{\mathrm{Cr}}^{+3}/\mathrm{Cr}}^0=-0.74 \mathrm{V}$

Electrode potential data of a few cells is given below. Based on the data, arrange the ions in increasing order of their reducing power:
${\mathrm{Fe}}_{\left(\mathrm{aq}\right)}^{3+}+{\mathrm{e}}^{-}\to {\mathrm{Fe}}^{2+}{}_{\left(\mathrm{aq}\right)}; \mathrm{E}°=+0.77 \mathrm{V}$
${\mathrm{Al}}^{3+}{}_{\left(\mathrm{aq}\right)}+3{\mathrm{e}}^{-}\to {\mathrm{Al}}_{\left(\mathrm{s}\right)}; \mathrm{E}°=-1.66 \mathrm{V}$
${\mathrm{Br}}_{2\left(\mathrm{aq}\right)}+2{\mathrm{e}}^{-}\to 2{\mathrm{Br}}_{\left(\mathrm{aq}\right)}^{-}; \mathrm{E}°=+1.09 \mathrm{V}$

Which of the following reaction is not feasible :-
 

The standard electrode potential of three metals $\mathrm{X}, \mathrm{Y}$and $\mathrm{Z}$ are $-1.2 \mathrm{V}, +0.5 \mathrm{V}$ and $-3.0 \mathrm{V}$ respectively. The reducing power of these metals will be

A gas $\mathrm{X}$ at $1 \mathrm{atm}$ is bubbled through a solution containing a mixture of $1\mathrm{M} {\mathrm{Y}}^{-}$ and $1\mathrm{M} {\mathrm{Z}}^{-}$ ions at $25°\mathrm{C}$. If the reduction potentials of $\mathrm{Z}>\mathrm{Y}>\mathrm{X}$, then

If the half cell reactions are given as
(i) ${\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{–}\to \mathrm{Fe}\left(\mathrm{s}\right); \mathrm{E}°=–0.44\mathrm{V}$
(ii) $2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{–}\to {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); \mathrm{E}°=+1.23\mathrm{V}$
The $\mathrm{E}°$ for the reaction, $\mathrm{Fe}\left(\mathrm{s}\right)+2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ is

The ${\mathrm{E}}_{{\mathrm{M}}^{3+}/{\mathrm{M}}^{2+}}^{\mathrm{o}}$ values for $\mathrm{Cr},\mathrm{Mn},\mathrm{Fe}$ and $\mathrm{Co}$ are $-0.41,+1.57,+0.77$ and $+1.97\mathrm{V}$, respectively. For which one of these metals the change in oxidation state from $+2$ to $+3$ is the easiest?

Standard electrode potential of three metals $\mathrm{A},\mathrm{B}$ and $\mathrm{C}$ are $+0.5 \mathrm{V},-3.0 \mathrm{V}$ and $-1.2 \mathrm{V}$ respectively. The reducing power of these metals are

During electrolysis, the reaction at the anode is:

Which statement is true for an electrochemical cell?

The negative sign in the standard electrode potential indicates- 

As per study of electrochemical series, which of the following reaction is non-spontaneous?

A gas $\mathrm{X}$ at $1\mathrm{ }\mathrm{atm}$ is bubbled through a solution containing a mixture of $1\mathrm{ }\mathrm{M}\mathrm{ }{\mathrm{Y}}^{-}$ and $1\mathrm{ }\mathrm{M}\mathrm{ }{\mathrm{Z}}^{-}$ at $25 °\mathrm{C}$. If the reduction potential of $\mathrm{Z}>\mathrm{Y}>\mathrm{X}$, then

A gas $\mathrm{X}$ at $1 \mathrm{atm}$ is bubbled through a solution containing a mixture of $1 \mathrm{M} {\mathrm{y}}^{-}$ and $1 \mathrm{M} {\mathrm{z}}^{-}$ at $25\mathrm{℃}$. If the order of reduction potential is $\mathrm{z}>\mathrm{y}>\mathrm{x}$, then

Four alkali metals $A, B, C$and $D$ are having respectively standard electrode potential as $-3.05, -1.66, -0.40 \mathrm{a}\mathrm{n}\mathrm{d}\mathrm{ }0.80.$ Which one will be the most reactive?

Reduction potentials of four elements $\text{P,}\text{Q,}\text{R,}\text{S}$ is $-\text{2}\text{.90}\text{V}$, $\text{0.34}\text{V}$, $\text{1}\text{.2}\text{V}$ and $-\text{0}\text{.76}\text{V}$. The decreasing order of reducing power is

The standard electrode potential of hydrogen electrode at 1 M concentration and hydrogen gas at 1atm pressure is

${\mathrm{E}}_{\mathrm{Cu}}^{°}=0.34\mathrm{ }\mathrm{V}$ and ${\mathrm{E}}_{\mathrm{Zn}}^{°}\mathrm{ }=\mathrm{ }0.76\mathrm{ }\mathrm{V}.$ A Daniel cell contains $0.1 \mathrm{M} \mathrm{Z}\mathrm{n}\mathrm{S}{\mathrm{O}}_4$ solution and $0.01 \mathrm{M} \mathrm{C}\mathrm{u}\mathrm{S}{\mathrm{O}}_4$ solution at its electrodes. EMF of the cell is