The following is a portion of the Reduction Potential Table from your text (Tabl

Question

The following is a portion of the Reduction Potential Table from your text (Table 18.1, Zumdahl), with half-reactions ordered as described in the Introduction to this experiment. half-reaction +3eMnO2 + 2 H,0 02 + 2H2O + 4e-. Cr3+ 3eCr Li +e Li a. Which species is the reducing agent in the first half-reaction? b. Which species in the table is the strongest reducing agent? c. Which species in the table is the strongest oxidizing agent? d. Is the reaction of Cr with MnO, to produce Cr and MnO, spontaneous? e. Write the balanced chemical equation for the reaction of Cr" with Li. (Take into account the discussion on p. 123.)

Explanation / Answer

a)

reducing agnet --> must be oxidized easily, then this must be Li(s)(

b)

strongest reducing Agent --> form the list, Li(s)

c)

strongest oxidizing Agent --> will reduce readily, in tihs case MnO4-

d)

Cr = will be oxidized by MnO4- due to the potentials

which yield Cr+3 and mnO2

therefore, this is in fct spontaneous

e)

Cr+3(aq) + Li(s) = Li+(aq) + Cr(s)

balance charge

Cr+3(aq) + 3Li(s) = 3Li+(aq) + Cr(s)

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