How to Calculate the Mass of Iron(III) Oxide from 500g of Iron?

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To calculate the mass of iron(III) oxide produced from 500g of iron, start by writing the balanced chemical equation for the reaction between iron and oxygen. Use stoichiometry to determine the molar ratios of iron to iron(III) oxide. Convert the mass of iron to moles, then apply the molar ratio to find the corresponding moles of iron(III) oxide. Finally, convert the moles of iron(III) oxide back to mass using its molar mass. Understanding these steps is crucial for accurate calculations in gravimetric stoichiometry.
nic.harv
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gravimetric stoichiomerty... eh? HELP

calculate the mass of iron(III) oxide (rust) produced by the reaction of 500g of iron with oxygen from the air

so i have no idea what do do here, my teacher sucks monkeys balls.



so i thought to do the mass of iron(III) oxide divided by the 500g but i know that's wrong. PLEASE HELP ME! I actually have no idea of what I am suppose to do.
 
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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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