How do you find the empirical formula of magnesium oxide, when magnesium ribbon is burned in a crucible...and a $0.91*g$ of material is present?

Md Ariful Islam

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Md Ariful Islam

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We need (i) the tare mass of the crucible;

(ii) the mass of the crucible and the magnesium metal BEFORE the reaction;

(iii) the mass of the crucible and the resultant magnesium oxide AFTER the rxn.

We interrogate the reaction:

$Mg(s) + 1/2O_2(g) rarr MgO$

And thus we need the mass of the metal, and the mass of the metal oxide. Do you have $0.91*g$ of metal or $0.91*g$ of metal oxide? We need BOTH masses to work out the .

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