Question

Represent the galvanic cell in which the reaction,

Zn(s) + Cu2+ (aq) -----→ Zn2+(aq) + Cu (s) takes place.​

Answer 1

Answer:

The galvanic cell in which the given reaction takes place is depicted as:

(i) Zn electrode (anode) is negatively charged.

 

(ii) Ions are carriers of current in the cell and in the external circuit, current will flow from silver to zinc.

 

(iii) The reaction taking place at the anode is given by,

Zn(s)  →   Zn2+(aq) + 2e-

The reaction taking place at the cathode is given by,

Ag+(aq)  + e-  →  Ag(s)

Answer 2

Answer:

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12th

Chemistry

Electrochemistry

Galvanic Cells

Represent the galvanic cell...

CHEMISTRY

Represent the galvanic cell in which the reaction takes place.

Zn(s)+Cu

2+

(aq)→Zn

2+

(aq)+Cu(s)

MEDIUM

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ANSWER

Measure the difference between the potentials of two electrodes that dip into the same solution, or more usefully, are in two different solutions. In the latter case, each electrode-solution pair constitutes an oxidation-reduction half cell, and we are measuring the sum of the two half-cell potentials.

This arrangement is called a galvanic cell. A typical cell might consist of two pieces of metal, one zinc and the other copper, each immersed each in a solution containing a dissolved salt of the corresponding metal. The two solutions are separated by a porous barrier that prevents them from rapidly mixing but allows ions to diffuse through.

If we connect the zinc and copper by means of a metallic conductor, the excess electrons that remain when Zn

2+

ions emerge from the zinc in the left cell would be able to flow through the external circuit and into the right electrode, where they could be delivered to the Cu

2+

ions which become "discharged", that is, converted into Cu atoms at the surface of the copper electrode. The net reaction is the oxidation of zinc by copper(II) ions:

Zn

(S)

+Cu

(aq)

2+

⟶Zn

(aq)

2+

+Cu

(s)