Calculate the emf of the cell with the cell reaction
`Ni _((s))+2Ag ^(+)(0.002M)to Ni^(2+)(0.160M) +2 Ag_((s))`
`E_(cell)^(0)=1.05V.`

If E_(cell)^(@) is 1.05 V, the emf of the cell for the following cell reaction Ni(s)+2Ag^(+)(0.004 M) rarr Ni^(2+)(0.16M)+2Ag(s) at 298 K in V is

The emf of the cell in which of the following reaction , Zn_((s)) +Ni^(2+) (0.1 M) to Zn^(2+) (1.0M) + Ni_((s)) occurs is found to 0.5105 V at 298 K . The standard emf of the cell is

Represent the cell in which the following reaction takes place Mg(s)+2Ag^(+)(0.0001M) to Mg^(2+) (0.130M)+2Ag(s) Calculates its E_(cell) if E_("cell")^(Θ)=3.17V

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

Calculate the emf of the cell consisting the following half cells Al//Al^(3+)(0.001M), Ni//Ni^(2)(0.50M). Given that E_(Ni^(2+)//Ni)^(0)=-0.25V E_(Al^(3+)//Al)=-1.66V(log 8xx10^(-6)=-5.0969).

Determine the values of K_(c) for the following reacton Ni_((s))+2 Ag _((aq))^(+)to Ni_((aq))^(2+)+2Ag _((s)) E^(0) =1.05V.

Calculate the equilibrium constant of the reaction : Cu_((s))+2Ag_((aq))^(+)to Cu_((aq))^(2+)+2Ag_((a)) E_((cell))^(Θ)=0.46V

Calculate Delta G^(@) for the following cell reaction. Zn_((s)) + Ag_(2)O_((s)) + H_(2)O((I)) to Zn_(aq)^(2+) + 2Ag(s) + 2OH_((aq))^(-) E_((Ag^(+))/(Ag))^(@) =+0.80V and E_((Zn^(2+))/(Zn)) ^(@)=-0.76V

Calculate the emf of the cell at 298 K Sn_((s))|Sn^(2+)(0.05M)||H_((aq))^(+)(0.02M) |H_(2) 1 atm. Pt Given that E_(sn^(2+)//Sn)^(0)=-0.144V

What is the reaction quotient , Q for the cell Ni_((s)) | Ni^(2+) (0.190 M) || Cl^(-) (0.40 M) | Pt_((s)) Cl_(2(g)) (1.0 atm)