Question

Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 3 Mg N2 → Mg3N2 In a particular experiment, a 8.33-g sample of N2 reacts completely. The mass of Mg consumed is ________ g.

Answer 1

Answer:

The mass of Mg consumed is 21.42g

Explanation:

The reaction is

$3Mg+N_{2}-->Mg_{3}N_{2}$

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 = $\frac{mass}{molarmass}=\frac{8.33}{28}=0.2975mol$

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