How many grams of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg (s) ? Show all calculations leading to an answer. List 3 indicators of a chemical change.

Balanced chemical reaction happening here is:

3Mg (s) + N₂ (g) → Mg₃N₂ (s)

moles of product formed from each reactant:

2.0 mol of N2 (g) x 1 mol Mg₃N₂ = 2 mol Mg₃N₂

1 mol N2

and

8.0 mol of Mg (s) x 1 mol Mg₃N₂ = 2.67 mol Mg₃N₂

3 mol Mg

Since N2 is giving the least amount of product (Mg₃N₂) ie. 2 mol Mg₃N₂

N2 is the limiting reactant here and Mg is excess reactant.

Hence mole of product formed here is 2 mol Mg₃N₂

molar mass of Mg₃N₂

= 3 Mg + 2 N

= 101g/mol

mass of product (Mg₃N₂) formed

= moles x Molar mass

= 2 x 101

= 202g Mg₃N₂

202g of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg (s).

The following are indicators of chemical changes:

Change in Temperature

Change in Color

Formation of a Precipitate