Calculate the emf and DeltaGof cell reaction for the following cell at 25 °C : Mg(s) | Mg^(2+) (0.001 M) || Cu^(2+) (0.0001 M) + Cu(s) [E_(Mg^(2+)//Mg)]^(@) = -2.37 V, E_(Cu^(2+)//Cu)^(@) =+0.34 V and 1F = 96500C mol^(-1)

Calculate the emf and DeltaGof cell reaction for the following cell at

1.	Calculate the emf and DeltaGof cell reaction for the following cell at 25 °C : Mg(s) \| Mg^(2+) (0.001 M) \|\| Cu^(2+) (0.0001 M) + Cu(s) [E_(Mg^(2+)//Mg)]^(@) = -2.37 V, E_(Cu^(2+)//Cu)^(@) =+0.34 V and 1F = 96500C mol^(-1)
Answer» Solution :The following reactions take place in the cell: `Mg(s) to Mg^(2+) (aq) + 2e^(-)` `Cu^(2+) (aq) + 2e^(-) to Cu(s)` `Mg(s) + Cu^(2+) (aq) to Mg^(2+) (aq) + Cu(s)` Thus, n=2 APPLYING Nernst equation and substituting the values, we GET `E_("cell") = E_(Cu^(2+)//Cu)^(@) -E_(Mg^(2+)//Mg)^(@) -0.0591/2 LOG ([Mg^(2+)])/([Cu^(2+)])` `=0.34 V - (-2.37 V) - 0.0591/2 log 0.001/0.0001` `=2.71 V - 0.0591/2 log 10 = 2.71 V - 0.0295 V = 2.6805V` `DeltaG` can be OBTAINED as under: `DeltaG = -nFE =-2 xx 2.6805 xx 96500` `=-517336.5 J mol^(-1) = -517.34 kJ mol^(-1)`