Emf of the cell
`Ni| Ni^(2+) ( 0.1 M) | Au^(3+) (1.0M)` Au will be
`E_(Ni//Ni(2+))^@ = 0.5=25. E_(Au//Au^(3+))^@ = 1.5 V`.

Emf of the cell Ni|Ni^(2+) (0.1M)||Au^(3+) (1.0M)|Au will be (Given E_(Ni^(2+)//Ni)^(@)= 0.25V, E_(Au^(2+)//Au)^(@)= 1.5V )

emf of cell Ni, Ni^(2+)(1.0M) || Au^(3+)(1.0M), Au is …………If E^@ for Ni^(2+)|Ni is 0.25V, E^@ for Au^(3+)| Au is 1.50 V.

Calculate the standard electrode potential of Ni^(2+) | Ni electrode if emf of the cell, Ni(s) | Ni^(2+) ( 0.01 M ) || Cu^(2+) ( 0.1M) | Cu(s) is 0.059 V. [ Given E_(Cu^(2+) //Cu) ^(@) = + 0.34V

Calculate the emf and write the chemical reaction for the cell constructed with AI|AI^(3+)(0.01 M) and NI|Ni^(2+)(0.2 M) , E_(Ni^(2+)//Ni)^@ =-0.25V E_(AI^(3+)//AI)^@ =-1.66V

The cell emf for the cell Ni(s)abs(Ni^(2+)(1.0M))Au^(3+)(1.0M)| Au(s) (E^(o) for Ni^(2+) abs(Ni=-0.25 V,E^(o)" for " Au^(3+))Au=1.50V) is

The cell emf for the cell Ni(s)abs(Ni^(2+)(1.0M))Au^(3+)(1.0M)| Au(s) (E^(o) for Ni^(2+) abs(Ni=-0.25 V,E^(o)" for " Au^(3+))Au=1.50V) is