Write the cell reaction taking plce in the cell CU_((s))|Cu_((aq))^(+2)||Ag _((aq))^(+) |Ag _((s))
The cell reaction of the galvanic cell, Cu(s) // Cu^(2+)(aq) // Hg^(2+) (aq) // Hg (l) is
Write the Nernst equation for the EMF of the cell Ni _((s))|Ni +_((aq))^(2+)||Ag_((aq))^(+)|Ag
Calculate the emf of the cell Cu(s) | Cu^(2+) (aq) || Ag^(+)(aq) | Ag(s) Given, E_((Cu^(2+))//(Cu))=+ 0.34 V, E_((Ag^(+))//( Ag)) = 0.80 V
The cell reaction of a cell is Mg(s) + Cu^(2+)(aq) to Cu(s) + Mg^(2+)(aq) If the standard reduction potentials of magensium and copper are -0.33 and +2.38 V respectively, the emf of the cell is
The value of the reaction quotient ,Q for the cell Zn(s) |Zn^(2+) (0.01M)||Ag^(+)(1.25M)|Ag(s) is :
Depict the galvanic cell in which the reaction Zn(s) + 2Ag^(+) (aq) to Zn^(2+) (aq) + 2A(s) takes place. Further show. (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.
Which metal will dissolve if the cell works Cu|Cu^(2+)||Ag^(+)|Ag