Asked by Ari

The following is a Limiting Reactant problem: Magnesium nitride is formed in the reaction of magnesium metal with nitrogen gas in this reaction: 3 Mg(s) + N2(g) -> Mg3N2(s)

How many grams of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg(s)?
Answered by Devin
Do you have any choices or is it one where you answer it with what you know?
Answered by Devin
Mole Ratio of Mg : Mg3N2 = 3 b: 1

mole of Mg3N2 = moleofmagnesium over 3 = 8.0mol over 3 = 2.67 mol

mass of Mg3N2 = mole * molar mass = 2.67 mol * ((3* 24) + (2 * 14)) g / mol = 2.66.67

I hope that helped you out :)
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