Nitrogen is present in excess.
<h3>What is the no. of moles of nitrogen?</h3>
3Mg + N2 = Mg3N2
Moles of Mg = mass / molar mass = 2.22 / 24.3 = 0.0914
Moles of N2 = 3.75 / 28=0.1339
In conclusion, as we produce less amount of M g3N 2 when we assumed that M g was the limiting reagent, magnesium is the limiting reagent and nitrogen is the excess.
<h3>How can magnesium nitride be made through a direct reaction?</h3>
The elements can directly react to form magnesium nitride, as demonstrated in the equation 3 mg (s)+n2 (g)=Mg3N2 (s).
<h3>What is excess reactant?</h3>
Reactants that are not totally consumed are referred to as "excess reactants," whereas reactants that are completely consumed or reacted are referred to as "limited reactants." How much of the limiting reactants are consumed determines how much product is generated. In this section, the definition of excess reactant, examples, and calculations are discussed.
Learn more about magnesium nitride:
brainly.com/question/20980092
#SPJ4
