Question

In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above...

In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Yb2+Yb + 2Yb3+

Will Yb2+ disproportionate in aqueous solution?

To justify your answer, what is the standard cell voltage for the disproportionation reaction? V

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Answer #1

The given reaction is

3Yb2+(aq) = Yb(s) + 2Yb3+(aq)

In a disproportionation reaction, an element undergoes both oxidation and reduction.

Oxidation number of Yb in 3Yb2+ = +2

Oxidation number of Yb = 0

Oxidation number of Yb in 2Yb3+ = +3

Yb is reduced from +2 to 0

Yb is oxidized from +2 to +3

Yb acts an oxidizing agent and reducing agent in a single reaction.

The given reaction is disproportionation reaction.

Reduction reaction

Yb2+ + 2e- = Yb

Ered = - 2.76 V

Oxidation reaction

Yb2+ = Yb3+ + e-

Eox = 1.05 V

Standard reduction potential

E°cell = Eox + Ered

= 1.05 - 2.76

= - 1.71 V

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