Electrochemistr...

A Voltaic cell consists of an electrode of solid silver immersed in 0.10M $${ AgNO }_{ 3 }$$ Solution and an electrode of unknown metal X immersed in a 0.10M solution $${ X(NO }_{ 3 })_{ 2 }$$. A porous barrier separates the two half of the cell. Also given:

$$E\left( { Ag^{ + } }/{ Ag } \right)$$ = 0.80V and $${ E }_{ cell }$$ = 1.05V and at 25 degree Celsius

$${ X_{ (s) } }/{ { X }^{ 2+ } }(1.0M)\parallel { Ag }^{ + }(0.1M)/{ Ag }_{ (s) }$$

Which of the following statements regarding the cell and X is correct?

For a cell reaction represented by the equation $$Cu(s)+2Ag^{+}(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)$$ the value of $$\Delta G^{\circ}$$ could be obtained by 

Which one of the following metals could not be obtained on electrolysis of aqueous solution of its salts ?

Number of electrons lost during electrolysis of 0.355 g of $$Cl^-$$ is:

Without losing its concentration $$ZnCl_2$$ solution cannot be kept in contact with :

$${{\text{E}}^{\text{o}}}_{{\text{C}}{{\text{u}}^{{\text{2 + }}}}{\text{|Cu = }}}\,{\text{ + 0}}{\text{.337}}\,{\text{V}}\,$$, $${{\text{E}}^{\text{o}}}_{{\text{Z}}{{\text{n}}^{{\text{2 + }}}}{\text{|Zn = }}}\,{\text{-0.762}}\, {\text{V}}\,$$ The EMF of the cell, $${\text{Zn|Z}}{{\text{n}}^{{\text{2 + }}}}\left( {{\text{0}}{\text{.1M}}} \right)||\,{\text{C}}{{\text{u}}^{{\text{2 + }}}}\left( {{\text{0}}{\text{.01M}}} \right){\text{|Cu}}$$ is :

On the basis of the following $$E^0$$ the strongest oxidising agent is:
$$\begin{array}{l}{\left[ {Fe{{\left( {CN} \right)}_6}} \right]^{4 - }} \to {\left[ {Fe{{\left( {CN} \right)}_6}} \right]^{3 - }} + {e^ - };{E^0} =  - 0.35V\\F{e^{2 + }} \to F{e^{3 + }} + {e^ - };{E^0} =  - 0.77V\end{array}$$ 

An amino acid migrates towards the cathode when the electric field is applied. This implies that 

$$\frac{1}{2}F_{2}+e^{-}\rightarrow F^{-};\ E^{\circ}=+3.02V$$