Consider the cell:
`Mg(s)|Mg^(2+)(0.13M)||Ag^(+)(1.0xx10^(-4))M|Ag(s)`
its e.m.f. is `2.96V.` calculate `E_("cell")^(@)`
`(R=8.314JK^(-1),1F=96500Cmol^(-1))`

Calculate the e.m.f. of the following cell at 298 K, Mg|Mg^(2+)(0.130M)||Ag^(+)(1.0xx10^(-4)M)|Ag

Calculate the emf of the following cell at 298K: Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1.0xx10^(-3)M)|Cu(s) [Given= E_(Cell)^(@)=2.71V ]

Calculate the cell potential for the cell, Ni(s)//Ni^(2+)(0.1 M) || Ag^(+)(0.1 M)//Ag(s) ["Given",E_(Ag^(+)//Ag)^(@)=+0.80" V ", E_(Ni^(2+)//Ni)^(@)=-0.25" V ", R=8.314 JK^(-1) mol^(-1),F=96500 C mol^(-1)]

The e.m.f of the cell Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1xx10^-xM)|Cu is 2.651 V. The standard e.m.f of the cell is 2.71 V. the value of x is

Calculate the cell emf and triangle_(r)G^(@) for the cell reactin at 25^(@)C Zn(s)|Zn^(2+)(0.1M)||Cd^(2+)(0.01M)|Cd(s) (given E_(Zn^(2+)//Zn)^(@)=-0.763V,E_(Cd^(2+)//Cd)^(@)=-0.403V 1F=96500Cmol^(-1),R=8.314JK^(-1)mol^(-1)]

Calculate the e.m.f. and DeltaG for the cell reaction at 298 K: Mg_((s))"/"Mg_((0.1M))^(2+)"//"Cu_((0.01M))^(2+)"/"Cu_((s)) Given E_("cell")^(@) = -2.71V 1F=96,500C