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1 September, 03:16

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

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  1. 1 September, 03:29
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    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.
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