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:

Fe₃N₂ + F₂ → Fe₃F₂ + N₂.

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).

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.

where is the following

explanation:

the answer is 303.15 or 303