Answer:
The mass of Mg consumed is 21.42g
Explanation:
The reaction is
[tex]3Mg+N_{2}-->Mg_{3}N_{2}[/tex]
As per balanced equation, three moles of Mg will react with one mole of nitrogen to give one mole of magnesium nitride.
as given that mass of nitrogen reacted = 8.33g
So moles of nitrogen reacted = [tex]\frac{mass}{molarmass}=\frac{8.33}{28}=0.2975mol[/tex]
moles of Mg required = 3 X moles of nitrogen taken = 3X0.2975 = 0.8925mol
Mass of Mg required = moles X molar mass = 0.8925 X 24 = 21.42 g
