How Do You Calculate the Empirical Formula from Element Percentages?

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To calculate the empirical formula from element percentages, divide the percentage of each element by its respective atomic mass. This gives the number of moles for each element. Next, find the simplest whole number ratio of these mole values. For example, if you have three elements, perform these calculations for each to derive the empirical formula. This method effectively determines the compound's empirical formula based on its elemental composition.
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If i have percenteges of three elements, making up a compound, how do i Calculate the molecular formula or empirical formula of the compound? Can someone give me an example?
 
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to calculate the empirical formula,u have to divide the % with the elements respective Ar then find the simple ratio.
 
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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