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    Nooooooooooooooooooooooooooo

    :cry2:
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    ffs

    wai
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    (Original post by Pandora.)
    Nooooooooooooooooooooooooooo

    :cry2:
    Haha! :party2:

    :console:
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    (Original post by Felix Felicis)
    ffs

    wai
    What a shame :console:
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    (Original post by Felix Felicis)
    ffs

    wai
    :console: Life's tough man...

    (Original post by usycool1)
    Haha! :party2:

    :console:
    I hope you're pleased with yourself :hmmm:

    My brother think Nadal won't win tomorrow.

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    Rafa.


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    Was hoping for an all swiss final :/

    Can only hope Djokovic/ Wawrinka take it now

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    I was so excited for a moment there, thinking that I could go to uni in London just to stalk a certain GOAT.

    Alas, I think it's too late.. :moon:
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    Dear Chemists!

    So I got rate equation:
    Rate=k[ClO2]^2[OH-]

    And my question is:
    How does it provide evidence that the reaction takes place by more than one step?
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    (Original post by purplemind)
    Dear Chemists!

    So I got rate equation:
    Rate=k[ClO2]^2[OH-]

    And my question is:
    How does it provide evidence that the reaction takes place by more than one step?
    Second order? No idea, just felt like saying something because it looks so good
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    (Original post by L'Evil Fish)
    Second order? No idea, just felt like saying something because it looks so good
    I had to work out orders in a previous part so I'm afraid stating that the order is second wouldn't be enough.
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    (Original post by purplemind)
    Dear Chemists!

    So I got rate equation:
    Rate=k[ClO2]^2[OH-]

    And my question is:
    How does it provide evidence that the reaction takes place by more than one step?
    Were you given the "actual" equation for the reaction?
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    (Original post by purplemind)
    Dear Chemists!

    So I got rate equation:
    Rate=k[ClO2]^2[OH-]

    And my question is:
    How does it provide evidence that the reaction takes place by more than one step?
    Have they given you any other information?
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    (Original post by purplemind)
    I had to work out orders in a previous part so I'm afraid stating that the order is second wouldn't be enough.
    Oh, there actually are orders?:lol: I'm just saying random stuff. Can't wait for A2
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    (Original post by usycool1)
    Were you given the "actual" equation for the reaction?
    (Original post by mynameisntbobk)
    Have they given you any other information?
    So from previous parts I know that:
    Rate=k[ClO2]^2[OH-]
    and k=200.

    Later they tell me that 'In the overall equation, 2 mol ClO2 reacts with 2 mol OH- to form an aqueous solution containing chlorate (III) and chlorate (V) ions.

    I found the overall equation: 2ClO2 + 2OH- -> ClO2- + ClO3- + H2O

    (I thought this information isn't important because they asked how the rate equation provides evidence that reaction takes place by more than 1 step).

    (Original post by L'Evil Fish)
    Oh, there actually are orders?:lol: I'm just saying random stuff. Can't wait for A2
    I'm doing OCR Chemistry A but I guess syllabus is similiar for all exam boards. But I don't find it too interesting (maybe that's because Chemistry isn't my favourite subject. )
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    (Original post by mynameisntbobk)
    Congrats dude some hefty grades though I'm sure you'll manage it

    (Original post by furryface12)
    :woo: Well done! Good luck with those grades though


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    (Original post by Lucy96)

    Yay congratulations!
    (Original post by Prinz655)
    well done
    Thanks guys
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    (Original post by adi19956)
    Thanks guys
    Ooh, I've just seen - well done! :awesome:
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    (Original post by purplemind)
    So from previous parts I know that:
    Rate=k[ClO2]^2[OH-]
    and k=200.

    Later they tell me that 'In the obverall equation, 2 mol ClO2 reacts with 2 mol OH- to form an aqueous solution containing chlorate (III) and chlorate (V) ions.

    I found the overall equation: 2ClO2 + 2OH- -> ClO2- + ClO3- + H2O

    (I thought this information isn't important because they asked how the rate equation provides evidence that reaction takes place by more than 1 step).
    I'm not actually sure. I'd probably guess it has something to do with the fact that the orders of the reactant are different (?)
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    (Original post by purplemind)
    So from previous parts I know that:
    Rate=k[ClO2]^2[OH-]
    and k=200.

    Later they tell me that 'In the overall equation, 2 mol ClO2 reacts with 2 mol OH- to form an aqueous solution containing chlorate (III) and chlorate (V) ions.

    I found the overall equation: 2ClO2 + 2OH- -> ClO2- + ClO3- + H2O

    (I thought this information isn't important because they asked how the rate equation provides evidence that reaction takes place by more than 1 step).
    Hmm...not 100% sure. If you're asked to just use the rate equation, all I can think of is that the rate equation shows only the rate-determining step (i.e. the slowest step in the reaction) and so there must be more than one step. Not 100% sure though tbh :holmes:
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    (Original post by adi19956)
    Thanks guys
    Congrats!!
 
 
 
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