Chemical Kinetics QuestionDetermination of order of reaction

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SUMMARY

The discussion centers on the determination of the order of reaction for the decomposition of N2O5, represented by the equation 2N2O5(g) --> 4NO2(g) + O2(g). The user initially interprets the linear plot of pressure (P(N2O5)) against time (t) with a negative slope as indicative of zero-order kinetics. However, the correct classification is first-order kinetics, as the plot of ln[P(N2O5)] versus time would yield a negative slope, aligning with the textbook answer. This highlights the importance of understanding the relationship between concentration, pressure, and reaction order in chemical kinetics.

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nishantve1
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Homework Statement



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 ?

Homework Equations





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
 
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