Is My Calculation of NO2 Production Accurate?

AI Thread Summary
The discussion centers on the calculation of NO2 production from the decomposition of N2O5, specifically questioning the accuracy of a result of 9.30 g NO2 produced from 1.618 g of O2. The user applied molar conversions using the molecular weights of O2 and NO2, following the balanced equation. While the outlined steps for the calculation are acknowledged as correct, the specific calculations have not been verified by others in the thread. The inquiry seeks confirmation of the final result and the methodology used. Accurate calculations are crucial for understanding stoichiometric relationships in chemical reactions.
ldixon
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2N2O5 heat-- 4NO2 + O2

1.618 g of O2 are produced, how much NO2 in grams are produced? I got 9.30 g NO2, is that right? I used 1 mol O2 = 32 g O2, and 1 mol NO2 = 46g NO2. I first converted g O2 to Mol O2 then used the balanced equation to convert from mol O2 to mol NO2, then converted to NO2 to grams. If anyone can tell me if I did this right I would greatly appreciate it.
 
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The steps that you outlined are good, however I haven't checked your calculations specifically.
 
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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