Electrochemical Cells

Explain the chemical reaction occurring in the methanol fuel cell. 

Write the half cell reactions occurring in the methanol fuel cell.

Give the cathodic and anodic reaction occuring during the electrolysis of molten lead bromide.

Explain the electrolysis of molten lead(II) bromide.

Sketch the cell for the electrolysis of molten $\mathrm{NaCl}$. Indicate cathode, anode and their signs. Show the flow of electrons and ions.

Describe the electrolysis of molten $\mathrm{NaCl}$ using inert electrodes.

Sketch the cell for electrolysis of molten ${\mathrm{MgCl}}_2$. Indicate anode, cathode with their signs. Show the direction of electron and ion flow. Write electrode reactions and net cell reaction.

Write shorthand notation for the cell of the following reaction:

${\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right)$ is oxidized by ${\mathrm{Br}}_2\left(\mathrm{l}\right)$

Write shorthand notation for the cell of the following reaction:

${\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)+2{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)⟶\mathrm{Cu}\left(\mathrm{s}\right)+2\mathrm{AgBr}\left(\mathrm{s}\right)$

Formulate a cell from the following electrode reactions:
$\left(\mathrm{a}\right) {\mathrm{Cl}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}⟶2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$

$\left(\mathrm{b}\right) 2{\mathrm{I}}^{-}\left(\mathrm{aq}\right)⟶{\mathrm{I}}_2\left(\mathrm{s}\right)+2{\mathrm{e}}^{-}$

Formulate a cell for each of the following reactions: 

$\left(\mathrm{b}\right) \mathrm{Mg}\left(\mathrm{s}\right)+ {\mathrm{Br}}_2\left(\mathrm{l}\right) \to {\mathrm{Mg}}^{2+}\left(\mathrm{aq}\right)+ 2{\mathrm{Br}}^{-}\left(\mathrm{aq}\right)$

Formulate a cell for each of the following reactions:

(a) ${\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{AgCl}\left(\mathrm{s}\right)\to {\mathrm{Sn}}^{4+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)+2\mathrm{Cl}-\left(\mathrm{aq}\right)$

What are the conventions used to write cell diagram (cell formula)?
 

The following redox reaction occurs in a galvanic cell.

$2\mathrm{Al}\left(\mathrm{s}\right)+3{\mathrm{Fe}}^{2+}\left(1\mathrm{M}\right)⟶2{\mathrm{Al}}^{3+}\left(1\mathrm{M}\right)+3\mathrm{Fe}$

Write the cell notation.

$\mathrm{Pb}\left(\mathrm{s}\right)\mid {\mathrm{Pb}}^{2+}\left(1\mathrm{M}\right)\Vert \mathrm{KCl}\left|{\mathrm{Hg}}_2{\mathrm{Cl}}_2\left(\mathrm{s}\right)\right|\mathrm{Hg}\left(\mathrm{s}\right)$

Identify anode and cathode. Name the right hand side electrode.

Give some examples of metals which can be extracted electrochemically?

Which of the following is used in electroplating of iron seat?

How many coulombs are required for the oxidation of one mole of ${\mathrm{H}}_2\mathrm{O}$ to${\mathrm{O}}_2$?

During electrolysis, the positive ions move towards the