Question about heating an oxide

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Allowing fumes to escape during the initial heating in the formation of magnesium oxide would lead to an underestimation of the amount of magnesium oxide produced. This is because the escaping fumes likely contain oxygen, which is a necessary reactant in the reaction between magnesium and oxygen to form magnesium oxide. If oxygen is lost, the reaction will not proceed to completion, resulting in a lower yield of magnesium oxide than expected. Consequently, this would introduce a calculation error in determining the stoichiometry of the reaction and the final mass of magnesium oxide produced.
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I have this post lab question that I am not sure how to answer...
What error in calculation would result if, in the procedure for forming the magnesium oxide, the fumes in the intial heating were allowed to escape?
Any help would be great! Thanks!
 
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Hello,

Magnesium oxide is produced from magnesium powder (or wire, the physical structure is not important) and oxygen gas:

Mg + \frac {1}{2}~O_2 \xrightarrow {heat} MgO

The initial fumes are probably oxygen gas, the inevitable reactant to convert to the oxide. I think you got the point already. The rest is up to you.
 

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