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Question
Represent a cell consisting of Mg2+ | Mg half cell and Ag+
| Ag half cell and write the cell reaction.
( `"E"_("Ag")^° = 0.799 "V", "E"_("Mg")^° = - 2.37 "V"`)
Solution
The given data indicates that Mg undergoes oxidation and Ag+ undergoes reduction. Hence, cell reaction is
`"Mg(s)" -> "Mg"_("aq")^(2+) + 2e^-` ...(Oxidation half reaction at anode)
`"2Ag"_("aq")^+ + 2e^- -> 2"Ag"_("s")` ...(Reduction half reaction at cathode)
____________________________________________________________________
`"Mg"_("s") + 2"Ag"_("aq")^+ -> "Mg"_("aq")^2+ + 2"Ag"_("s")` ...(Overall cell reaction)
The cell representation is
`"Mg"_("s") | "Mg"_("aq")^(2+) ( xx "M" ) || "Ag"_("aq")^+ ( y M) | "Ag"_("s")`
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