What is standard cell potential for the reaction `3Ni (s) + 2Al^(3+)(1M)rarr3Ni^(2o+)(1M) + 2Al(s)` if `E_(Ni)^0 =- 0.25 V` and `E_(AI)^0 = -1.66V`?

What is standard cell potential for the reaction Cell notation 3Ni(s) + 2AI^(3o+) (1M) rarr 3Ni^(2o+) (1M) + 1Al(s) if E_(Ni)^@ =-0.25 V and E_(AI)^0 =-1.66V?

The standard potential for the cell reaction 2Ti_((S)) + Hg^(2+) (1M) rarr 2Ti^+ (1 M) + Hg_((I)) Where E_(Ti)^@ =- 0.34V, E_(Hg)^@ = 0.86 V is

Calculate equilibrium constant for the reaction, Ni_((s)) + 2Ag_((aq))^(2+) rarr Ni_((aq))^(2+) + 2Ag_((s)) at 25^@C E_(Ni)^@ =- 0.25V and E_(Ag)^@ = 0.799V .

For the reaction Ni(s) + Cu^(2o+)(1M) rarr Ni^(2o+)(1M) + Cu (s), E^@ cell = 0.57 V DeltaG^@ of the reaction is

Calculate standard Gibbs energy change and equilibrium constant at 25^@C for the cell reaction, Cd (s) + Sn^(2o+) (aq) rarr Cd^(2o+) (aq) + Sn (s) Given : E_(Cd)^@ = -0.403V and E_(Sn)^@ = -0.136 V . Write formula of the cell.

Write the cell reaction and calculate the standard potential of the cell. Ni_((s))|Ni^(2+) (M)||CI (1M)|CI_2 (g.latm)|Pt E_(Cl2)^@ = 1.36 V and E_^@ = -0.25 V

The standard potential of the cell in which the following reaction occurs H_2 (g,1atm) + Cu^(2o+)(1M)rarr2H^(o+)(1M)+Cu(S), ( E^0Cu = 0.34V) is

Calculate E_(cell)^@, DeltaG^@ and equilibrium constant for the reaction : 2Cu_((aq))^+ rarr Cu_((aq))^(2+)+ Cu_((s)) E_(Cu+//Cu)^@=0.52V and E_(Cu+/Cu)^@=0.16V

Arrange the following oxidizing agents in order of increasing strength under standard state conditions.The standard potentials for the reduction half reaction are given: CI_(2(g)) (1.36V), I_2(s) (0.54V), Cd_((aq))^(2+) (-0.4V)

Consider the following redox reaction Mg_((s))+Sn_(aq)^(2+) rarr Mg^2+ Sn_((s)) Calculate E_(cell) for the reaction at 25^@C if [Mg^(2+)] = 0.035M, [Sn^(2+)] = 0.025M , E_(Mg)^0 =- 2.37V and E_(Sn)^0 =-0.136V .