Question

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)?

Answer 1

since you know both the amounts of \(N_2\) and \(Mg\) you start with, compare the mole ratio that the balanced reaction says you \(need\) with the molar amounts the problem says you \(have\)

Answer 2

the balanced reaction tells you that for every 1 mole of \(N_2\), you \(need\) three times that much \(Mg\) in order to use everything up

You \(have\) two moles of \(N_2\), so how many moles of \(Mg\) should be used?