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    Why is the answer D and not A?
    And what do they mean "against the square of the concentration of a reactant ..?"
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    (Original post by Adorable98)
    Why is the answer D and not A?
    And what do they mean "against the square of the concentration of a reactant ..?"
    hmmmm a very interesting question ...
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    (Original post by charco)
    hmmmm a very interesting question ...
    So you don;t know the answer?
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    (Original post by Adorable98)
    So you don;t know the answer?
    no, I don't know the question!
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    (Original post by charco)
    no, I don't know the question!
    I'm going to have a guess even though we don't know what's 'in the box'.

    The answer is D because the reaction is second order with respect to the reactant in question and therefore is squared in the rate equation.

    Your go!
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    (Original post by TeachChemistry)
    I'm going to have a guess even though we don't know what's 'in the box'.

    The answer is D because the reaction is second order with respect to the reactant in question and therefore is squared in the rate equation.

    Your go!
    I still don't get it.
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    (Original post by Adorable98)
    I still don't get it.
    Aha, an image has appeared ...

    D is a straight line which shows direct proportionality between rate and the concept on the other axis.

    This is only possible if

    rate = k x [A]2

    or

    rate = k[A][ B]
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    (Original post by charco)
    Aha, an image has appeared ...

    D is a straight line which shows direct proportionality between rate and the concept on the other axis.

    This is only possible if

    rate = k x [A]2

    or

    rate = k[A][ B]
    Oh, I see!! Thank you!!
 
 
 
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