Use the table \'Standard Reduction Potentials\' located in the \'Tables\', to pr

Question

Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Pb metal is put into a 1M aqueous Sn2+solution.

If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.

Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Ni metal is put into a 1M aqueous Cr3+solution.

If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.

Explanation / Answer

1)

from data table:

Eo(Sn2+/Sn(s)) = -0.130

Eo(Pb2+/Pb(s)) = -0.126

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

here:

cathode is (Pb2+/Pb(s))

anode is (Sn2+/Sn(s))

The chemical reaction taking place will be

Pb2+ + Sn(s) --> Pb(s) + Sn2+

But this is not what we want

Reaction will not occur

2)

from data table:

Eo(Cr3+/Cr(s)) = -0.740

Eo(Ni2+/Ni(s)) = -0.250

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

here:

cathode is (Ni2+/Ni(s))

anode is (Cr3+/Cr(s))

The chemical reaction taking place will be

Ni2+ + Cr(s) --> Ni(s) + Cr3+

But this is not what we want

Reaction will not occur

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