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)?
2 answers
Do you have any choices or is it one where you answer it with what you know?
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 :)
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 :)