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)?

mole ratio of   Mg : Mg₃N₂   =  3 b:  1

∴  mole of  Mg₃N₂ =  
                  
                              =  
                        
                              =  2.67 mol

mass of Mg₃N₂  =  mole  *  molar mass
                          =  2.67 mol  *  ((3 * 24) + (2 * 14)) g / mol
                          =  266.67 g

Are there any options?

The correct answer is b