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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.

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closed as off-topic by Todd Minehardt, airhuff, MaxW, andselisk, M.A.R. ಠ_ಠ Dec 26 '17 at 10:27

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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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