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.

The mass of Mg consumed is 21.42g

Explanation:

The reaction is

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 =

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

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