Question

A galvanic^cell consists of left ompartmcnt with a tin elcctrode in contact with 0.1 M Sn(NO_3)_2(aq) and a right compartment with a lead electrode in contact with 1 times l0^-3 M Pb(NO_3)_2(aq). The relevant reduction potentials are: When this cell is allowed to discharge spontaneously at 25 degree C, which of the following statements is true?

a) Electrons will flow from left to right through the wire.
b) Pb^2+ ions will be reduccd to Pb metal.
c) The concentration of Sn2+ ions in the left compartment will increase.
d) The tin electrode will be the cathodc.
e) No noticeable change will occur, bccausc the cell is a. eqmhbnum.

Answer 1

Electrons will flow from left to right through the wire.

Pb^2+ ions will be reduccd to Pb metal.

The concentration of Sn2+ ions in the left compartment will increase.

Step-by-step explanation:

Looking at the relative electrode potentials of the two metals

Sn= -0.14

Pb=-0.13

Tin is expected to function as the anode (left hand half cell) and lead as the anode (right hand half cell) tin oxidizes to sn^2+ hence its concentration increases on the left compartment while lead is reduced to ordinary lead metal on the right hand half cell . since oxidation occurs on the left hand side, electrons flow from left to right.