Question

Briefly explain how the Mg to O ratio would have been affected if you had failed to convert all of the MG₃N₂ present to magnesium oxide.

Answer 1

The initial value

Mg3N2(s) --> MgO(s) + N2(g)

we need to addd O2(g) for oxidatio nto occur

balance

2Mg2N2 + O2 = MgO + N2

now, balance

2Mg3N2 + 3O2 → 6MgO + 2N2

ratio is we fail Mg3N2 vs MgO

if we fail to convert all

There will be present:

Mg3N2 --> MW = 100.9284 g/mol

MgO --> MW = 40.3044 g/mol

In the end, we will assume most of this is MgO

then Mg3N2 will be an impurity

This will increase the mass of our sample

which will lower our ratio

Since

Total Mg species = Mg3N2 and MgO

Mg higher in ratio in Mg3N2 tan MgO

therefore, the ratio is Mg >> O