Question

nsider the following reaction : 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 anod

Answer 1

1. Cu to Ag
2. anod Cu =Cu2+
3. cethod 2 Ag+ = 2Ag

Answer 2

i) $Cu/Cu^{2+}//Ag^+/Ag$

ii) copper to silver.

iii)$2Ag^+(aq)+2e^-\rightarrow 2Ag(s)$

$Cu(s)\rightarrow Cu^{2+}(aq)+2e^-$

Explanation:

The representation is given by writing the anode on left hand side followed by its ion with its molar concentration. It is followed by a salt bridge. Then the cathodic ion with its molar concentration is written and then the cathode.

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

ii) Here Cu undergoes oxidation by loss of electrons, thus act as anode. Silver undergoes reduction by gain of electrons and thus act as cathode.Thus electrons flow from copper to silver.

iii) Cathode : reduction : $2Ag^+(aq)+2e^-\rightarrow 2Ag(s)$

Anode: Oxidation : $Cu(s)\rightarrow Cu^{2+}(aq)+2e^-$

Learn more about electrochemical cell

https://brainly.in/question/2967160

https://brainly.in/question/7155939