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Thread: Balancing a redox equation

  1. #1 Balancing a redox equation 
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    Having trouble balancing this equation:

    I2 + ClO- --> I- + ClO3-

    Here is what I have for oxidation numbers:

    I2 + ClO- --> I- + ClO3-
    Oxidation Numbers 0 +1 -2 -1 +5 -2








    This is what I have so far:

    2I2 + ClO- --> 4I- + ClO3-


    I can't work out what to do for the ClO parts.

    Any help would be awesome.


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  3. #2  
    Bullshit Intolerant PhDemon's Avatar
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    Where did you get this reaction from? It can't be balanced with just those species...


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  4. #3  
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    I know. It's homework.
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  5. #4  
    Forum Junior AndresKiani's Avatar
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    ? Did a reaction even take place here? Lol
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  6. #5  
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    What am I looking at....
    I can never know I'm right, but I can know that I'm wrong.
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  7. #6  
    KJW
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    One often finds in redox reactions the requirement of species such as H+, OH, and H2O (indicating the pH-dependence of the redox reaction). In balancing the reaction, it can be useful to obtain the balanced redox half-reactions.
    There are no paradoxes in relativity, just people's misunderstandings of it.
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  8. #7  
    Forum Junior AndresKiani's Avatar
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    Quote Originally Posted by JackAnimated View Post
    Having trouble balancing this equation:

    I2 + ClO- --> I- + ClO3-

    Here is what I have for oxidation numbers:

    I2 + ClO- --> I- + ClO3-
    Oxidation Numbers +1 -2 -1 +5 -2








    This is what I have so far:

    2I2 + ClO- --> 4I- + ClO3-


    I can't work out what to do for the ClO parts.

    Any help would be awesome.
    If a reaction doesn't take place than electrons cannot be transferred for there to be a reducing and oxidizing effect. Maybe your teacher wanted you to add the missing reactants.. Otherwise you couldn't transfer those electrons.
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