Question

A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Mn(s) and Mn2+(aq). What species are produced at the electrodes under standard conditions? Ag+(aq) + e- → Ag(s) E° = +0.80 V Mn2+(aq) + 2 e- → Mn(s) E° = -1.18 V A) Ag(aq) is formed at the cathode and, Mn(s) is formed at the anode. B) Ag(s) is formed at the cathode, and Mn2+(aq) is formed at the anode. C) Mn(s) is formed at the cathode, and Ag+(aq) is formed at the anode. D) Mn2+(aq) is formed at the cathode, and Ag(s) is formed at the anode.

Answer 1

Answer: B) Ag(s) is formed at the cathode, and
`Mn^(2+)(aq)` is formed at the anode.

Step-by-step explanation:

`Ag^(+)(aq)+e^(-1)\rightarrow Ag(s)` E=0.80 V

`Mn^(2+)(aq)+2e^(-1)\rightarrow Mn(s)` E=-1.18 V

Reduction takes place easily if the standard reduction potential is higher (positive) and oxidation takes place easily if the standard reduction potential is less(more negative).

Thus as reduction potential of Ag is higher , it undergoes reduction and Manganese with lower reduction potential undergoes oxidation. Here Mn undergoes oxidation by loss of electrons, thus act as anode. Ag undergoes reduction by gain of electrons and thus act as cathode.

Cathode : reduction :
`Ag^(+)(aq)+e^(-1)\rightarrow Ag(s)`

Anode : oxidation :
`Mn\rightarrow Mn^(2+)(aq)+2e^(-1)`

Ag(s) is formed at the cathode, and
`Mn^(2+)(aq)` is formed at the anode.