Question

Cu(s) + 2ag+ (aq)  2ag(s) + cu2+(aq) (i) depict the galvanic cell in which the given reaction takes place. (ii) give the direction of flow of current. (iii) write the half-cell reactions taking place at cathode and anode.

Answer 1

Galvanic cell

Ag | Ag ²+ || Cu ²+ | cu

half cell reactions

Ag —> Ag ²+ + 2 e-

Cu²+ + 2e- —> Cu

Answer 2

(i)  Galvanic cell is $Cu/Cu^{2+} || Ag^{+}/Ag$.

(ii) Flow of current is from cathode to anode.

(iii) Oxidation-half reaction: $Cu \rightarrow Cu^{2+} + 2e^{-}$

Reduction-half reaction: $Ag^{+} + 1e^{-} \rightarrow Ag$

Explanation:

It is known that the flow of current is always opposite to the flow of electrons.

(i)   For the given reaction the expression for galvanic cell is as follows.

                $Cu/Cu^{2+} || Ag^{+}/Ag$

(ii)  As here occurs a decrease in the oxidation state of Ag. So, this means silver is reducing and since, there is an increase in the oxidation state of copper. So, this means that oxidation of copper is taking place.

And, electrons will flow from anode(oxidation) to cathode(reduction). Therefore, flow of current will be from cathode to anode.

(iii) The half-cell reactions for given reaction is as follows.

Oxidation-half reaction: $Cu \rightarrow Cu^{2+} + 2e^{-}$

Reduction-half reaction: $Ag^{+} + 1e^{-} \rightarrow Ag$

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