Calculate the standard electrode potential of Ni2+/Ni electrode if emf of the cell Ni |Ni2+(0.01 M)||Cu2+(0.1 M)| Cu(s) is 0.59 V at 25°C [Given: Ecu2+Icu = +0.34 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 potential (EMF) of the cell Cd/ Cd2+ (0.01M) ||H+(0.02M) | H (0.5 atm) given E° for Cd2+/Cd = -0.40V

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)

Calculate the reduction potential of the following electrode at 298K Pt,Cl_2(2.5atm)|HCl(0.01M), E^@ Cl_2|2Cl^-=1.36V .

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

Calculate the electrode potential of a silver electrode dipped in a 0.1 M solution of silver nitrate at 298K assuming AgNO_3 to be completely dissociated. The standard electrode potential of Ag^+|Ag is 0.80V at 298K.

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

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