Question

In: Chemistry

Decide whether or not each metal dissolves in 1 molL−1HCl(aq). Reduction Half-Reaction E∘(V) Al3+(aq)+3e− →Al(s) -1.66...

Decide whether or not each metal dissolves in 1 molL−1HCl(aq). Reduction Half-Reaction E∘(V)

Al3+(aq)+3e− →Al(s) -1.66

Mg2+(aq)+2e− →Mg(s) -2.37

Ag+(aq)+e− →Ag(s) 0.80

Au3+(aq)+3e− →Au(s) 1.50

Pb2+(aq)+2e− →Pb(s) -0.13

Cd2+(aq)+2e− →Cd(s) -0.40

Will

a) Al

dissolves
does not dissolve

b) Ag

dissolves
does not dissolve

c) Pb

dissolves
does not dissolve

Solutions

Expert Solution

Al3+ will dissolve

Mg2+ will dissolve

Ag+ will not dissolve

Au3+ will not dissolve

Pb2+ will dissolve

Cd2+ will dissolve

Theory

Reduction potential of H is 0.00V

Suppose reduction potential of metal ion is negative comparing to Hydrogen reduction potential then the metal will dissolve.For example take Al3+

E0 = - 1.66V, supppose Aluminium dissolve in HCl then this will be anode and H+ to H2 reduction electrode is cathode. Now,

E0(Cell ) = E0(Cathode) - E0(anode)

= 0.00V - (-1.66)

= +1.66V

So ,there is a driving force to dissolve Aluminium in HCl and the cell is operative

Suppose, If we take Ag as example

E0(cell) = 0.00V -(0.80 V)

= -0.80V

Negative volt indicate cell is not operative and Ag will not dissolve in HCl

queen_honey_blossom answered 2 years ago
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