If you have 78.50 grams of Fe3N2 reacts with 15.67 grams of F2, How many grams of each product can be made?

82.21 g of Fe₃F₂ and 11,2 g of N₂.

Explanation:

The reaction between Fe₃N₂ and F₂ is represented as:

Fe₃N₂ + F₂ → Fe₃F₂ + N₂.

it is clear that 1.0 mole of Fe₃N₂ reacts with 1.0 mole of F₂ to produce 1.0 mole of Fe₃F₂ and 1.0 mole of N₂. We need to calculate the no. of moles of Fe₃N₂ (78.50 g) and F₂ (15.67 g) using the relation:

n = mass/molar mass,

n of Fe₃N₂ = mass/molar mass = (78.50 g) / (195.5484 g/mol) = 0.4 mol.

n of F₂ = mass/molar mass = (15.67 g) / (37.99681 g/mol) = 0.41 mol ≅ 0.4 mol.

∴ Fe₃N₂ reacts with F₂ with a (1:1) molar ratio.

So, the products will be Fe₃F₂ (0.4 mol) and N₂ (0.4 mol).

Now, we can get the masses of each product using the relation:

mass = n x molar mass.

∴ mass of Fe₃F₂ = n x molar mass = (0.4 mol) (205.5318 g/mol) = 82.21 g.

∴ mass of N₂ = n x molar mass = (0.4 mol) (28.0 g/mol) = 11,2 g.