Question

Consider the conproportionation reaction between MnO4–(aq) and Mn2+(aq) leading to MnO2(s). (a) Balance the conproportionation reaction...

Consider the conproportionation reaction between MnO4–(aq) and Mn2+(aq) leading to MnO2(s).

(a) Balance the conproportionation reaction in acidic media using smallest whole number coefficients.

(b) Explain the meaning behind, “conproportionation.”

(c) Evaluate ∆Eo (V) for the conproportionation reaction in (a). The standard reduction potential between MnO4–(aq) and MnO2(s) is +1.68 V.

(d) Is this conproportionation reaction spontaneous? (Yes/No) Explain your choice.

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Answer #1

b) Conproportionation is a chemical reaction where two reactants, each containing the same element but in different oxidation states react to form a product in which the common element involved has the same oxidation number.

In the reaction between MnO4- and Mn++ ,the common element is Mn. The Oxidation number of Mn in MnO4- is +7 and in Mn++ is +2. They react to produce the same product MnO2 in which the oxidation number of Mn is +4. This oxiation number is intermediate between +7 and +2 .

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