Galvanic or Voltaic Cells

The reaction occurs in which of the given galvanic cell?

$\frac{1}{2}{\mathrm{H}}_2( \mathrm{g})+\mathrm{AgCl}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)+\mathrm{Ag}\left(\mathrm{s}\right)$

Draw a neat labelled diagram of galvanic cell which converts energy of combustion of fuels.

Which one of the following statements is TRUE for the galvanic cell?

If agar agar prevents intermixing of fluids then how does the $\mathrm{KCl}$ ions migrate ?

Derive the correct cell representation for the given cell reaction?

$\mathrm{Zn}+{\mathrm{H}}_2{\mathrm{SO}}_4\to {\mathrm{ZnSO}}_4+{\mathrm{H}}_2$

Consider the following equation for an electrochemical cell reaction. Which of the following changes in condition will increase the cell voltage? ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{PbCl}}_2\left(\mathrm{s}\right)\to \mathrm{Pb}\left(\mathrm{s}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)$
(I) Dissolve concentrated ${\mathrm{HClO}}_4$ in the cell solution
(II) Increase the pressure of ${\mathrm{H}}_2\left(\mathrm{g}\right)$
(III) Increase the amount of $\mathrm{Pb}\left(\mathrm{s}\right)$

The no. of cells which may be constructed with different ${\mathrm{E}}_{\mathrm{Cell}}°$ values for the reaction: $\mathrm{Fe}+2{\mathrm{Fe}}^{3+}\to 3{\mathrm{Fe}}^{2+}$

What are galvanic cell? Describe the construction and working of Daniel cell and the reaction involved. How is it represented?

Consider the following reaction: $\mathrm{Cu}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\to 2\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)$. 

Depict the galvanic cell in which the given reaction takes place.

Explain the function of salt bridge in an electrochemical cell.

What is an electrochemical cell? Describe the working of Daniel cell.

A hypothetical electrochemical cell is $\mathrm{A}/{\mathrm{A}}^{+}\left(\mathrm{x} \mathrm{M}\right)\parallel {\mathrm{B}}^{+}\left(\mathrm{y} \mathrm{M}\right)/\mathrm{B}$. The emf measured is $+0.20 \mathrm{V}$. The cell reaction is 

Write the cell formulation and calculate the standard cell potential of the galvanic cell in operation of which the reaction taking place is:

$2\mathrm{Cr}\left(\mathrm{s}\right)+3{\mathrm{Cd}}^{2+}\left(\mathrm{aq}\right)\stackrel{ }{\to }2{\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+3\mathrm{Cd}\left(\mathrm{s}\right)$

Calculate the $△{\mathrm{G}}^{\circ }$ for the above reaction. (Given: ${{\mathrm{E}}^{\circ }}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}=-0.74 \mathrm{V}, {{\mathrm{E}}^{\circ }}_{{\mathrm{Cd}}^{2+}/\mathrm{Cd}}=-0.40 \mathrm{V}, \mathrm{F}=96500 \mathrm{C} {\mathrm{mol}}^{-1}$)

The zinc/silver oxide cell is used in hearing aids and electric watches. The following reaction takes place:

$\mathrm{Zn}\stackrel{ }{\to }{\mathrm{Zn}}^{2+}+2{\mathrm{e}}^{-}; {\mathrm{E}}^{\circ }=-0.76 \mathrm{V}$

${\mathrm{Ag}}_2\mathrm{O}+{\mathrm{H}}_2\mathrm{O}+2{\mathrm{e}}^{-}\stackrel{ }{\to }2\mathrm{Ag}+2{\mathrm{OH}}^{-}; {\mathrm{E}}^{\circ }=0.344 \mathrm{V}$

What is oxidised and what is reduced?

The ${\mathrm{E}}^{\circ }$ values corresponding to the following two reduction electrode processes are, 

(i) ${\mathrm{Cu}}^{+}/\mathrm{Cu}=+0.52 \mathrm{V}$ (ii) ${\mathrm{Cu}}^{2+}/{\mathrm{Cu}}^{+}=+0.16 \mathrm{V}$

Formulate the galvanic cell for their combination. What will be the standard cell potential for it? Calculate ${\mathrm{\Delta }}_{\mathrm{r}}\mathrm{G}°$ for the cell reaction. ($\mathrm{F}=96500 \mathrm{C} {\mathrm{mol}}^{-1}$)

${\mathrm{Cu}}^{2+}+2{\mathrm{e}}^{-}\stackrel{ }{\to }\mathrm{Cu}: {\mathrm{E}}^{°}=+0.34 \mathrm{V}; {\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}\stackrel{ }{\to }\mathrm{Ag}; {\mathrm{E}}^{°}=+0.80 \mathrm{V}$

Construct a galvanic cell using the above data.

A voltaic cell is set up at ${25}^{\mathrm{o}}\mathrm{C}$ with the half cells, $\mathrm{A}{\mathrm{l}}^{3+}\left(0.001\mathrm{}\mathrm{M}\right)$ and $\mathrm{N}{\mathrm{i}}^{2+}\left(0.50\mathrm{}\mathrm{M}\right)$
Write an equation for the reaction that occurs when the cell generates an electric current and determine the cell potential. (Given ${\mathrm{E}}_{\mathrm{N}{\mathrm{i}}^{2+}/\mathrm{N}\mathrm{i}}^0=-0.25\mathrm{V},\mathrm{}{\mathrm{E}}_{\mathrm{A}{\mathrm{l}}^{3+}/\mathrm{A}\mathrm{l}}^0=-1.66\mathrm{V}$)

 Represent the cell in which the following reaction takes place.The value of ${\mathrm{E}}^0$ for the cell is $1.260 \mathrm{V}$. What is the value of ${\mathrm{E}}_{\mathrm{cell}}$ ?

$2\mathrm{Al}\left(\mathrm{s}\right)+3{\mathrm{Cd}}^{2+}\left(0.1 \mathrm{M}\right)\stackrel{ }{\to }3\mathrm{Cd}\left(\mathrm{s}\right)+2{\mathrm{Al}}^{3+}\left(\mathrm{aq}\right)\left(0.01 \mathrm{M}\right)$

Discuss the effect if no salt bridge is used in the galvanic cell.

_____ reduces the liquid junction potential by releasing ions into the solution.