The following chemical Feaction is occurring in an electrochemical cell. `Mg(s) + 2 Ag^(+) (0.0001 M)rarr Mg^(2+) (0.10 M) + 2 Ag (s)` The `E^@` electrode values are `Mg^(2+)//Mg = -2.36 V` `Ag^(+)//Ag = 0.81 V` For this cell, calculate/write : Cell potential `E_(cell)` .

The following chemical Feaction is occurring in an electrochemical cell. Mg(s) + 2 Ag^(+) (0.0001 M)rarr Mg^(2+) (0.10 M) + 2 Ag (s) The E^@ electrode values are Mg^(2+)//Mg = -2.36 V Ag^(+)//Ag = 0.81 V For this cell, calculate/write : (i)Symbolic representation of the above cell. (ii) Will the above cell reaction be spontaneous?

Write each half cell reaction of the following electrochemical cell: Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag(s)

Mg(s)+2Ag^(+)(1M)rarrMg^(+2)(1M)+2Ag(s) Write cell representation for above reaction.

For an electrochemical cell Cu//Cu^(2+) (XM)||Ag^(+) (Ym)//Ag . The cell reaction is

Represent the cell in which the following reaction takes place Mg(s) + 2Ag^+(0.0001M) to Mg^(2+)(0.130M) + 2Ag(s) Calculate its E_(cell) if E_(cell) = 3.17 V.

Write Nernst equation and calculate e.m.f. of the cell at 298 k. Mg(s)|Mg^(2+)(0.001 M)||Cu^(2+)(0.0001M)|Cu(s)

calculate the e.m.f of the cell in which the following reaction takes place: Ni(s) +2Ag^(+) (0.002M)rarrNi^(2+) (0.160 M)+2Ag(s) Given that E_(cell)^o=1.05V

Calculate the emf of the cell in which the following reaction takes place: Ni(s) + 2Ag^+ (0.002 M) Ni^(2+) (0.160 M) + 2Ag(s) Given that E^V_(cell) = 1.05 V

Write Nernst equation and calculate e.m.f. of the following cell at 298 k. Mg(s)|Mg^(2+)(0.130M)||Ag^+(0.0001M)|Ag(s) Given E^o(Mg^(2+)//Mg)=-2.37 V E^o(Ag^(+)//Ag)=0.80 V (log 1.3=0.1130)