How to solve this compound question?

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To determine the grams of Fe and liters of O2 needed to produce 0.5 kg of Fe2O3, first, understand the reaction equation 2Fe + 3O2 -> 2Fe2O3. Calculate the moles of Fe2O3 from the mass, then use stoichiometry to find the required moles of Fe and O2 based on the balanced equation. The ideal gas law (PV=nRT) can convert gas volume to grams, with 22.4 liters per mole as a key conversion factor. Ultimately, the focus should be on calculating the moles of products and reactants needed for the reaction.
transgalactic
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i got this formula

<br /> 2Fe +3O_2 -&gt; 2FeO_3<br />

how many grams of Fe and litters of oxigen do i need
in order to get 0.5 kilogram of

<br /> Fe_2O_3<br />

i can find how much grams weighs each mole of each molecule?

i don't know how to do the rest

??
 
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ok i understand
3 moles of
<br /> O_2<br />
can react at most with 2 moles of Fehow do i transform the volume of a gas into grams?
 
pV=nRT, ideal gas equation.
 
ok by pst 22.4 litters for every mole of gas
i can find the weight of each mole
what now?
 
Now you start thinking on your own, we are not here to spoonfeed you.

How many moles of product?

How many moles of reactants needed?
 

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