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Activation energies of manganate ion reactions Watch

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    Hi, I was doing a titration and I was wondering why the activation energy for potassium permanganate reacting with the iron(II) ions is greater than the activation energy for potassium permanganate reacting with the ethanedioate ion.

    Is it because the manganate ion is negative and it more easily reacts with the posotive iron(II) ion needing little energy, but more energy is needed for manganate to react with the negative ethanedioate ion?
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    Hi, I was doing a titration and I was wondering why the activation energy for potassium permanganate reacting with the iron(II) ions is greater than the activation energy for potassium permanganate reacting with the ethanedioate ion.

    Is it because the manganate ion is negative and it more easily reacts with the posotive iron(II) ion needing little energy, but more energy is needed for manganate to react with the negative ethanedioate ion?
    If the activation energy is greater for KMnO4 with Iron (II) than for ethanedioate/oxalate ions then surely that means more energy is required to initiate the KMnO4 and Iron (II) reaction?
    (Unless you meant the other way around?)

    You're right about the positive charge with Iron (II) and the negativeness of the oxalate though, and not having a look at any notes that would seem a solid explanation otherwise.
 
 
 
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