Calculate the e.m.f. of the cell in which the following reaction takes place.
`Ni_((s)) + 2Ag_((0.002M))^(+) to Ni_((0.160M))^(2+) + 2Ag_((s)) , "Given " E_("cell")^@ = 1.05 V `

(a) Calculate the emf of the cell in which the following reaction takes place Ni(S) + 2Ag^(+)(0.002M) rarr Ni^(2+)(0.160M) + 2Ag(S) Given that E_(cell)^(circ)= 1.05V (b) A galvanic cell after use is recharged by passing current through it. What type of cell is it? Give an example.

Represent the cell in which the following reaction takes place Mg(s)+2Ag^(+)(0.001M) to Mg^(2+)(0.130)+2Ag(s) Calculate E_("cell")" if "E_("cell")^(0)=3.17V .

For a given data : E_(Mg^(2+) // Mg)^(@) = -2.37 V , E_(Cu^(2+)// Cu)^(@) = + 0.34 V Calculate the emf of the cell in which the following reaction takes place . underset((0.0001 M)) ( Mg_((s))) + Cu_((aq))^(2+) underset((0.001M)) to Mg_((aq))^(2+) + Cu_((s))

a) Calculate the e.m.f. of the cell represented below: Ni_((s))|Ni_(0.1M)^(2+)||Ag_(0.01M)^(+)|Ag_((s))" at 298 Given, "E_("cell")^(@)=1.05V ,

b) Calculate Delta_(r)G^(@) for the following reaction: Fe_((aq))^(+2)+Ag_((aq))^(+)rarr Fe_((aq))^(+3)+Ag(s)." "("Given : "E_("cell")^(@)=+0.03V, F=96500C) .