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  4. For a cell, the cell reaction is: Mg(s)+Cu2+(aq)→ Cu(s)+Mg2+(aq) If the standard reduction potentials of Mg and Cu are -2.37 and +0.34 V respectively, the emf of the cell is

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Q. For a cell, the cell reaction is : $ Mg(s)+C{{u}^{2+}}(aq)\to Cu(s)+M{{g}^{2+}}(aq) $ If the standard reduction potentials of Mg and Cu are -2.37 and +0.34 V respectively, the emf of the cell is

EAMCETEAMCET 1998Electrochemistry

Solution:

Cell reaction, $ Mg(s)+C{{u}^{2+}}(aq.)\to Cu(s)+M{{g}^{2+}}(aq.). $
In this equation Mg is oxidised and Cu is reduced. So, oxidation takes place at Mg electrode and reduction takes place at Cu electrode. EMF Of Cell
$ ={{E}_{cathode}}-{{E}_{anode}} $
$ ={{E}_{reduction}}-{{E}_{oxidation}} $
$ =0.34-(-2.37) $ $ =0.34+2.37=2.71\,V $