Mixture of Gases: Composition & Properties

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The discussion revolves around a participant's confusion regarding their gas mixture calculations, which do not align with the professor's provided answers. Despite the participant's confidence in their calculations, they seek confirmation from others. Responses indicate that the calculations appear correct, and the suggestion is made to consult the professor for clarification. Ultimately, the participant considers the possibility of an error on the professor's part. The conversation highlights the importance of verifying academic information and seeking expert advice.
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Attached is the question and my working, my answers don't match up to the given answers, but they still seem right. Can anybody see where the mistake is?
 

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Your calculations look alright to me but an expert's view on the matter will be definitely welcome. Have you asked your professor?
 
I don't see anything wrong about your numbers.
 
Ok thanks. The answers provided are the ones given by the professor, ill assume he has made an error.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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