Which of the following would identify the weakest reducing agent from the species in a table of electrode potentials?

To identify the weakest reducing agent from a set of species represented in a table of electrode potentials, one should focus on the values of the electrode potentials associated with each species. In electrochemistry, a reducing agent is a species that donates electrons in a redox reaction and, as such, has a tendency to be oxidized. The strength of a reducing agent can be inversely related to its electrode potential.

The electrode potential indicates the tendency of a species to gain electrons (be reduced). The species with the lowest electrode potential is less likely to gain electrons compared to others with higher potentials. This means that it is less effective at being reduced and thus corresponds to a weaker reducing agent, as it is more inclined to remain in its oxidized form instead of providing electrons.

In contrast, species with higher electrode potentials are stronger reducing agents, as they have greater tendencies to be reduced, thereby effectively donating more electrons. Therefore, selecting the species with the lowest electrode potential correctly identifies the weakest reducing agent based on the fundamental principles of electrochemical behavior.