Redox Reaction and Electrode Potential

The half equation for a redox reaction represents an equilibrium between two sides of an equation such as:
${\mathrm{Cu}}^{2+}{ }_{\left(\mathrm{aq}\right)} + 2{{e}}^{-} ---> \mathrm{Cu} \left(\mathrm{s}\right); {\mathrm{E}}^{\mathrm{o}}= +0.34 \mathrm{v}$

Will the conversion of ${\mathrm{Cu}}^{2+}$to $\mathrm{Cu}$ become more or less feasible if the concentration of ${\mathrm{Cu}}^{2+}$ increases? Give reason(s).

The half equation for a redox reaction represents an equilibrium between two sides of an equation such as:
${\mathrm{Cu}}^{2+}{ }_{\left(\mathrm{aq}\right)} + 2{\mathrm{e}}^{-} ---> \mathrm{Cu} \left(\mathrm{s}\right); {\mathrm{E}}^{\mathrm{o}}= +0.34 \mathrm{v}$

How will the value of ${\mathrm{E}}^{\mathrm{o}}$ change if the concentration of ${\mathrm{Cu}}^{2+}$ increases?

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 potential of $\mathrm{Z}>\mathrm{Y}>\mathrm{X}$, then

Which has the highest oxidising power?

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 

To determine the exact amount of acetic acid in a sample, $1.5\mathrm{g}$ of the sample is titrated against $0.5\mathrm{N}$ solution of $\mathrm{KOH}$. For the titration, $30\mathrm{mL}$ solution of $\mathrm{KOH}$ is required. The percentage content (weight wise) of acetic acid in the given sample is

Hypophosphorus acid is a good reducing agent because

Electrode potential depends upon

EMF of the given cell ${\mathrm{A}}_{\left(\mathrm{s}\right)}\left|{\mathrm{A}}_{\left(\mathrm{aq}\right)}^{2+}\right|\left|{\mathrm{B}}_{\left(\mathrm{aq}\right)}^{2+}\right|{\mathrm{B}}_{\left(\mathrm{s}\right)}$

Given ${\mathrm{E}}_{\mathrm{A}/{\mathrm{A}}^{2+}}^{\mathrm{o}}:+1.4\mathrm{V}$ and ${\mathrm{E}}_{\mathrm{B}/{\mathrm{B}}^{2+}}^{\mathrm{o}}:-1.4\mathrm{V}$

Find the incorrect statement

When iron is added to ${\mathrm{CuSO}}_4$ solution, copper is precipitated, it is due to

An iron wire is immersed in a solution containing ${\mathrm{ZnSO}}_4$ and ${\mathrm{NiSO}}_4$. When the concentration of each salt is $1\mathrm{M}$, predict which of the following reaction is likely to proceed.
Given ${\mathrm{E}}^{\mathrm{o}}\left({\mathrm{Zn}}^{+2}/\mathrm{Zn}\right)=-0.76 \mathrm{V}$
${\mathrm{E}}^{\mathrm{o}}\left({\mathrm{Fe}}^{+2}/\mathrm{Fe}\right)=-0.44 \mathrm{V}$
and ${\mathrm{E}}^{\mathrm{o}}({\mathrm{Ni}}^{+2}/\mathrm{Ni})=-0.25 \mathrm{V}$

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.

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

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