The equilibrium constant, K, is `2.0 xx 10^(19)` for the cell
`Ni(s) || Ni^(2+)(aq) || Hg_(2)^(2+)(aq) | Hg(l)`
The value of `E^(@)` at `25^(@)`C for this cell is closest to:

The cell reaction of the galvanic cell: Cu(s)|Cu^(2+)(aq)||Hg^(2+)(aq)|Hg(l) is

In the cell reaction: 2Al(s)+3NI^(2+)(aq)rarr2Al^(3+)(aq)+3Ni(s) The value of n is

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

E^(@) for the cell Zn(s)|Zn^(2+)(aq)|Cu^(2+)(aq)|Cu(s) is 1.1V at 25^(@)C the equilibrium constant for the cell reaction is about

The cell reaction of the galvanic cell, Cu(s) // Cu^(2+)(aq) // Hg^(2+) (aq) // Hg (l) is

E.M.F. of Ni(s) | Ni^(2+) (aq)||Cu^(2+) (aq)| Cu(s) cell can be increased by

For the voltaic cell respresents below Ni(s) | Ni^(2+)(aq) || Ag^(+)(aq) | Ag(s) Which change will increase the cell potential?

Given the equilibrium constant : K_(c) of the reaction : Cu(s) + 2Ag^(+)(aq) rightarrow Cu^(2+) (Aq) + 2Ag(s) is 10xx10^(15) , calculate the E_(cell)^(@) of this reaction at 298K . ([2.303 (RT)/(Ft) at 298K = 0.059V])

The equilibrium constant for the reaction Sr(s) +Mg^(+2)(aq)rarrSr^(+2)(aq)+Mg(s) is 2.69 xx 10^(12) at 25^(@)C . The E^(o) for a cell mad up of the Sr//Sr^(+2) and Mg^(+2)//Mg half cells