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Ch.19 - Electrochemistry
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.19 - ElectrochemistryProblema 55
Capitolo 19, Problema 55

Which metal could you use to reduce Mn2+ ions but not Mg2+ ions?

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1
Identify the reduction potentials of Mn^{2+} and Mg^{2+}.
Find a metal with a reduction potential between those of Mn^{2+} and Mg^{2+}.
Ensure the metal can reduce Mn^{2+} by having a more negative reduction potential than Mn^{2+}.
Check that the metal cannot reduce Mg^{2+} by having a less negative reduction potential than Mg^{2+}.
Select the appropriate metal based on these criteria.

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Reduction Potential

Reduction potential is a measure of the tendency of a chemical species to acquire electrons and be reduced. Metals with higher reduction potentials can reduce ions with lower reduction potentials. Understanding the standard reduction potentials of Mn2+ and Mg2+ is essential to determine which metal can reduce Mn2+ but not Mg2+.
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01:10
Standard Reduction Potentials

Electrochemical Series

The electrochemical series is a list of elements organized by their standard electrode potentials. It helps predict the feasibility of redox reactions. By comparing the positions of Mn2+ and Mg2+ in this series, one can identify which metals can reduce specific ions based on their relative potentials.
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02:46
Electrochemical Cells

Redox Reactions

Redox reactions involve the transfer of electrons between two species, where one is oxidized (loses electrons) and the other is reduced (gains electrons). Identifying the correct metal for the reduction of Mn2+ ions requires understanding the redox behavior of the metals in question and their ability to donate electrons in the reaction.
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03:12
Identifying Redox Reactions
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Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ni(s) + Zn2+(aq) → Ni2+(aq) + Zn(s)

b. Ni(s) + Pb2+(aq) → Ni2+(aq) + Pb(s)

c. Al(s) + 3 Ag+(aq) → Al3+(aq) + 3 Ag(s)

d. Pb(s) + Mn2+(aq) → Pb2+(aq) + Mn(s)

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