Determining the empirical formula of Magnesium Oxide

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If magnesium oxide smoke escapes during the experiment, the Mg:O ratio would decrease because there would be less magnesium present relative to oxygen. This is due to the loss of magnesium oxide, which affects the overall mass and ratio of the elements. The empirical formula remains MgO, but the specific ratio calculated from the experiment would reflect the loss. To demonstrate this mathematically, one would need to compare the initial and final masses of magnesium and oxygen. The conclusion is that the escape of magnesium oxide would lead to a decreased Mg:O ratio.
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Homework Statement


I already did the experiment but I'm trying to answer a question which asks"

Suppose that you allowed some magnesium oxide smoke to escape during the experiment. How would the Mg:O ratio have been affected? Would the ratio have decreased, increased or stayed the same? Explaine using calculations.


Homework Equations


I already know the empirical formula is MgO

The Attempt at a Solution


I think it will stay the same because you can't really reduce the ratio any furthur but I don't know how to show it using calculations. please help and thanks.
 
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bubbles1234 said:

Homework Statement


I already did the experiment but I'm trying to answer a question which asks"

Suppose that you allowed some magnesium oxide smoke to escape during the experiment. How would the Mg:O ratio have been affected? Would the ratio have decreased, increased or stayed the same? Explaine using calculations.


Homework Equations


I already know the empirical formula is MgO

The Attempt at a Solution


I think it will stay the same because you can't really reduce the ratio any furthur but I don't know how to show it using calculations. please help and thanks.

You are probably right however keep in mind that I do not know the context of the experiment.
 

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