When 0.313 g of Mg is heated strongly in a nitrogen (N2) atmosphere, a chemical reaction occurs. The product of the reaction weighs 0.433 g. Calculate the empirical formula of the compound containing Mg and N. Name the compound.

Mg₃N₂ (magnesium nitride)

Explanation:

M (total) = M (mg) + M (n)

M (n) = M (total) - M (mg)

= 0.433g - 0.313g

= 0.12g

mole (N) = 0.12g / 14.0067 g/mol

= 0.008567

mole Mg = 0.313g / 24.3050 g/mol

= 0.012878

Mg = 0.012878 / 0.008567

= 1.5

N = 0.008567 / 0.008567

= 1

multiply by 2 to get whole numbers

Mg = 1.5 * 2 = 3

N = 1 * 2 = 2

Mg₃N₂ (magnesium nitride)