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# Aluminum reacts with oxygen to give aluminum oxide.$$4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s})$$ What amount of $\mathrm{O}_{2},$ in moles, is needed for complete reaction with 6.0 mol of Al? What mass of $\mathrm{Al}_{2} \mathrm{O}_{3},$ in grams, can be produced?

## $4.5 \mathrm{~mol} \mathrm{O}_{2} ; 310 \mathrm{~g} \mathrm{Al}_{2} \mathrm{O}_{3}$

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and this problem were asked how many moles of oxygen are needed to complete a combustion reaction with six moles of aluminum and then were asked how many grams of aluminum oxide are produced. So the first thing we're gonna do is figure out how many moles of oxygen we need since we're told we're combusting six moles of aluminum and that is 1.5 times for aluminum. We can apply the same ratio to figure out how much oxygen we need. So it turns out we'll need 4.5 moles of Oxygen and the second part of the question were asked how many grams of aluminum oxide are produced. We can also calculate the molar mass of aluminum oxide, given the periodic table values for aluminum and oxygen, and we find that that value is 101.96 grams per mole. Knowing that we need three moles of aluminum oxide, we just most by three moles by this more mess and then we can get 306 grams of aluminum oxide are produced