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?

1 Answer
anor277
Apr 2, 2017

There are insufficient data here...........

Explanation:

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 stoichiometry.

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