use the table of standard reduction potentials to ecplain why iron will reduce copper but it...

use the table of standard reduction potentials to ecplain why iron will reduce copper but it will not reduce sodium

Solutions

Expert Solution

from data table:

Eo(Fe2+/Fe(s)) = -0.44 V

Eo(Cu2+/Cu(s)) = 0.337 V

the electrode with the greater Eo value will be reduced and it will be cathode

here:

cathode is (Cu2+/Cu(s))

anode is (Fe2+/Fe(s))

The chemical reaction taking place is

Cu2+(aq) + Fe(s) --> Cu(s) + Fe2+(aq)

Eocell = Eocathode - Eoanode

= (0.337) - (-0.44)

= 0.777 V

Since Eocell is positive, iron can reduce copper.

from data table:

Eo(Fe2+/Fe(s)) = -0.44 V

Eo(Na+/Na(s)) = -2.71 V

for given cell reaction to occur

cathode is (Na+/Na(s))

anode is (Fe2+/Fe(s))

Eocell = Eocathode - Eoanode

= (-2.71) - (-0.44)

= -2.27 V

Since Eocell is negative, iron can’t reduce copper.

queen_honey_blossom answered 1 year ago

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