Permanganate can be used to oxidize oxalic acid all the way to carbon dioxide. I

Question

Permanganate can be used to oxidize oxalic acid all the way to carbon dioxide. If you balance this redox reaction in acidic solution, which of the following statements about the balanced reaction is not true?

MnO4-(aq) + H2C2O4(aq) to Mn2+(aq) + CO2(aq)


a)The oxidation state of Mn changes from +7 to +2.
b)10 equivalents of CO2 are produced.
c)16 equivalents of H+ are required.
d)Each equivalent of MnO4- will react with 5 equivalents of oxalic acid.



NOTE:
I think its C or D.. before the reaction is balanced the equation DOES have H+, and there are 2MnO4- and 5 H2C2O4

so its a tricky question... heres my work to show what I mean:

10e- + 16H+ +2MnO4- + 5H2C2O4 to 2Mn2+ + 8H2O + 10CO2 + 10H+ + 10e-

and to simplify:

6H+ + 2MnO4- + 5H2C2O4 to 2Mn2+ + 8H2O + 10CO2

Explanation / Answer

"d" is wrong. (one MnO4^- to 2.5 oxalic acid) 2[MnO4^-] + 6H^+ + 5 H2C2O4 -----> 2Mn^+2 + 8H2O + 10CO2 so c is right

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