Mass of iron from the reduction of iron(III) oxide [closed]








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> 
> Given the equation
>  $$\ce{Fe2O3 + 3H2 -> 2Fe + 3H2O},$$
>  determine how many grams of $\ce{Fe}$ can be produced from $\pu{16.5 g}$ of $\ce{Fe2O3}$.
> 
> 
> 


I've already determined the masses of each component. I believe the next step is convert the masses into moles, but after that, I'm not sure what formula to use.


Any help is greatly appreciated.




After finding the moles of $\ce{Fe2O3}$ we see that after balancing the equation, $2$ moles of $\ce{Fe}$ are formed for every mole of $\ce{Fe2O3}$.


But that would be considering that the equation moves completely to the RHS, which is assumed if nothing is explicitly mentioned but not true.


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