Question 14.25 (Sixth Edition)

Moderators: Chem_Mod, Chem_Admin

Steve Magana 2I
Posts: 61
Joined: Fri Sep 28, 2018 12:24 am

Question 14.25 (Sixth Edition)

Postby Steve Magana 2I » Mon Feb 25, 2019 1:25 am

Question: Arrange the following metals in order of increasing strength as reducing agents for species in aqueous solution: (a) Cu, Zn, Cr, Fe; (b) Li, Na, K, Mg; (c) U, V, Ti, Al; (d) Ni, Sn, Au, Ag.

How does one determine the strength of each element in these cases? Thank you!

Elisa Bass 4L
Posts: 61
Joined: Fri Sep 28, 2018 12:23 am

Re: Question 14.25 (Sixth Edition)

Postby Elisa Bass 4L » Mon Feb 25, 2019 8:53 am

Remember that a metal having a more negative (or less positive) reduction potential means it is a stronger reducing agent (which means it is the species that is doing the reducing). For the first part of the problem, all the metals except Cu have negative reduction potentials, so compare those values with Cu having the lowest strength as a reduction agent.

Jordan Lo 2A
Posts: 85
Joined: Fri Sep 28, 2018 12:25 am

Re: Question 14.25 (Sixth Edition)

Postby Jordan Lo 2A » Mon Feb 25, 2019 10:25 am

A greater E on the standard reduction potential list means reduction is more favorable. For example, Lithium is a metal that likes to "give away" its electron so reducing it (adding an electron) is very unfavorable and E is very negative. When E is negative, the reverse reaction is more favorable

Aarti K Jain 1L
Posts: 30
Joined: Fri Sep 28, 2018 12:20 am

Re: Question 14.25 (Sixth Edition)

Postby Aarti K Jain 1L » Mon Feb 25, 2019 12:21 pm

The more negative the standard potential, the more strongly the reducing agent/element.

Return to “Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams”

Who is online

Users browsing this forum: No registered users and 8 guests