Question

Question 8.30 Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq)→Zn2+(aq) + 2Ag(s) takes place, further show:

(i) which of the electrode is negatively charged,

(ii) the carriers of the current in the cell, and

(iii) individual reaction at each electrode.

Class XI Redox Reactions Page 275

Answer 1

1) we know that anode is negatively charge.
Here Zn converts into Zn+2 ion(oxidation).
So Zn electrode is negatively charged.
2) ions are carriers of the current. 3) reaction on anode Zn(s) → Zn2+(aq) + 2e-
Reaction on cathode
Ag+(aq) + e- → Ag(s)
I think it will help u

Answer 2

the redox reaction for the galvanic cell is
Zn + 2Ag+ -------> Zn²+ + 2Ag
here, at anode Zn is oxidised to Zn²+ and at cathode Ag+ is reduced to Ag metal, Thus, Galvanic cell for the above redox reaction may be depicted as
Zn | Zn²+(aq) || Ag+(aq) | Ag

(i) Zn - electrode is negatively charged because the oxidation of Zn is increasing 0 to +2 {in Zn²+ ions} , hence, electrons are accumulated on Zinc electrode.

(ii) The ions carry current in the cell.we know, Current flows from higher potential to lower potential . it means current flows from Ag electrode to Zn electrode. while electrons flow from Zn electrode to Ag electrode.

(iii) individual reaction at each electrodes.
at anode : Zn -------> Zn²+ + 2e
at cathode: Ag+ + e ------> Ag