A voltaic cell is set up at `25^@C` with the given half cells: `Ag^+(0.001M)|Ag` and `Cu^(2+)(0.10M)|Cu`.
What would be the voltage of the cell `(E_(cell)^@=0.46V)`?

A voltaic cell is set up at 24^(@)C with the following half-cells AI^(3+)(0.001M) and Ni^(2+)(0.50M) . Write an equation for the reaction that occurs when the cell generates an electric current and determine the cell potential. (Given : E_(Ni^(2+)//Ni)^(@)=-0.25V,E_(Al^(3+)//Al)^(@)=-1.66V )

Derive Nernst equation for the following cell: Cu|Cu^(2+)(0.1M)||Ag^(+)(0*1M)|Ag

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.

For the cell, Tl|Tl^+(0.001)||Cu^(2+)(0.1M)|Cu , E_(cell) at 25^@C is 0.826V. The e.m.f can be increased

Write the Nernst equation and emf of the following cells at 298 K: Mg(s)|Mg^(2+)(0.001M) || Cu^(2+)(0.0001 M)| Cu(s)

Write Nernst equation and calculate emf for the following cell: Zn|Zn^(2+)(0*01M)||Ag^(+)(0*01M)|Ag .

Derive Nernst equation for the following cell: NiNi^(2+)(0*2M)||Cu^(2+)(0*2M)|Cu .

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

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 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