[Chris Houston]

Hey guys I have a quick question about this problem

Mg(s) + air ---> Mg x O y

1) If you start with .9g of Mg, determine the grams of solid that would result assuming 30% formed Magnesium Nitride instead of Mg Oxide

2)Also compare the mass above to the theoretical yield of MgO, if the nitride problem were ignored would the experimental ration of y to x be too high or too low?

I'm stumped any help would be appreciated. Thank you

[sjb]

Hey guys I have a quick question about this problem

Mg(s) + air ---> Mg x O y

1) If you start with .9g of Mg, determine the grams of solid that would result assuming 30% formed Magnesium Nitride instead of Mg Oxide

Does this mean 30% of the original magnesium formed the nitride, or that 30% (by weight? by moles?) of the new solid is the nitride? Seems a bit ambiguous to me

[Chris Houston]

I think it means 30% of the .9g of Mg formed Mg3N2

[sjb]

I think it means 30% of the .9g of Mg formed Mg3N2

OK, given that interpretation, write balanced equations for formation of oxide and nitride from magnesium, then see how much nitride you can form from 30% of 0.9 of Mg, and oxide from your remainder