For the reaction : `Ni(s)+2Ag^(+)(1M)rarrNi^(+2)(1M)+2Ag(s)`.
Which species get reduced?

calculate the e.m.f of the cell in which the following reaction takes place: Ni(s) +2Ag^(+) (0.002M)rarrNi^(2+) (0.160 M)+2Ag(s) Given that E_(cell)^o=1.05V

Mg(s)+2Ag^(+)(1M)rarrMg^(+2)(1M)+2Ag(s) Write cell representation for above reaction.

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

Depict the galvanic cell in which the reaction Zn(s)+2Ag^+(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show: Which of the electrode is negatively charged?

Depict the galvanic cell in which the reaction Zn(s)+2Ag^+(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show: The carriers of the current in the cell.

Calculate the equilibrium constant of the reaction: Cu(s) + 2Ag^+(aq) → Cu^(2+) (aq) + 2Ag(s) E^o(cell) = 0.46 V

In the reaction, SO_2(g) + 2H_2S (g) rarr 2H_2O (l) + S (s) the reducing agents is

Depict the galvanic cell in which the reaction Zn(s)+2Ag^+(aq) rarr Zn^(2+)(aq)+2Ag(s) takes place. Further show: Individual reaction at each electrode.

The following chemical Feaction is occurring in an electrochemical cell. Mg(s) + 2 Ag^(+) (0.0001 M)rarr Mg^(2+) (0.10 M) + 2 Ag (s) The E^@ electrode values are Mg^(2+)//Mg = -2.36 V Ag^(+)//Ag = 0.81 V For this cell, calculate/write : (i)Symbolic representation of the above cell. (ii) Will the above cell reaction be spontaneous?