Redox Reactions and Electrode Processes

For calculating the standard oxidation electrode potential, the reaction is carried out at $1 \mathrm{atm}$ pressure and $273 \mathrm{K}$ temperature. 

What are the two types of electrodes and give some examples.

What are the types of reactions that take place at the electrodes?

What are electrodes?

Define standard oxidation electrode potential.

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

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?

In the galvanic cell, which process occurs at the positive terminal, and what is it called?

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?

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

Aqueous ${\mathrm{Cu}}^{+}$ is unstable in solution and undergoes simultaneous oxidation and reduction according to the reaction

$2{\mathrm{Cu}}^{+}\mathrm{ }\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{Cu}}^{2+}\mathrm{ }\left(\mathrm{aq}\right)+\mathrm{Cu}\mathrm{ }\left(\mathrm{s}\right)$.

Choose the correct ${\mathrm{E}}^{°}$ for the above reaction.