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)?

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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)?

Chemistry
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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 \(have\)
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?

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