Calculate `E^@` For the cell :
`Al|Al^(3+)(1M)||Cu^(2+)(1M)Cu`
Given `E^@(Al^(3+)|Al)=-1.66V and `
`E^@(Cu^(2+) |Cu)=0.34V`

Calculate E^(@) for the cell : Al|Al^(3+)(1 M)||Cu^(2+)(1M)|Cu Given : E_(Al^(3+)//Al)^(@) and E_(Cu^(2+)//Cu)^(@) as -1.66 V and + 0.34 V respectively

(i) State Kohlrausch law. (ii) Calculate the emf of the following cell at 298 K: Al(s)//Al^(3+) (0.15M)//Cu^(2+)(0.025M) //Cu(s) (Given E^(@)(Al^(3+)//Al) = -1.66 V, E^(@)(Cu^(2+)//Cu) = 0.34V, log 0.15 = -0.8239, log 0.025 = - 1.6020)

Calculate Delta G^(Theta) and E_(cell) for the cell Al |Al^(3+) (0.01 M) || Fe^(2+) (0.02 M) |Fe Given that E_((Al^(3+)|Al))^(Theta) = -1.66 V and E_((Fe^(2+) |Fe))^(Theta) = -0.44 V

The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

Calculate the e.m.f of the cell Mg(s)//Mg^(2+)(0.1 M)||Cu^(2+)(1.0xx10^(-3) M)//Cu(s) Given E_(Cu^(2+)//Cu)^(@)=+0.34 V and E_(Mg^(2+)//Mg)^(@)=-2.37 V

The cell potential for the cell Ni|Ni^(2+)(1M)||Cu^(2+)(1M)|Cu is 0.59 V and E(Cu^(2+)|Cu) = +0.34 V . What is the standard electrode potential of Ni^(2+)|Ni electrode?

Calculate standard potential of cell E_(cell)^(0) by using E^(0)_(Al^(3+) | Al) and E_(Cu^(2+)| Cu )^(0) as –1.66V and + 0.34V respectively