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Chemical Kinetics Question . Determination of order of reaction

  1. Aug 13, 2012 #1
    1. The problem statement, all variables and given/known data

    So the question says
    for the reaction 2N2O5(g) --> 4NO2 (g) + O2(g) provides a linear plot when P(N205) is plotted against t with a negative slope . The decomposition of N2O5 follows ?

    2. Relevant equations

    3. The attempt at a solution
    I am guessing that P(N205) is pressure of N2O5 since for gases pressure is equivalent to Concentration so the plot will be between Concentration of N2O5 and time and the negative sloe would be -k the rate constant looking at this in my opinion the answer should be "zero-order kinetics" since for zero order kinetics plot between [A] and t has a negative slope .

    But the answer in the text is "First order kinetics" how ? I mean yes for first order the plot between ln[A] and time has a negative slope but how is that applicable in this case ?
    Thanks in advance
  2. jcsd
  3. Aug 13, 2012 #2


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    Gold Member

    Err... what can you say about the products?
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