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Nezavi [6.7K]
2 years ago
6

How many grams of Fe can be produced when 6.50 g of Fe2O3 reacts?

Chemistry
1 answer:
AveGali [126]2 years ago
6 0

Answer:

Mass of Fe produced = 4.468 g

Explanation:

Given data:

Mass of Fe produced = ?

Mass of Fe₂O₃ react = 6.50 g

Solution:

Chemical equation:

2Fe₂O₃        →     4Fe + 3O₂

Number of moles of Fe₂O₃ ;

Number of moles = mass/molar mass

Number of moles = 6.50 g/159.69 g/mol

Number of moles = 0.04 mol

Now we will compare the moles of iron and ironoxide.

                    Fe₂O₃             :             Fe

                         2                :              4

                       0.04             :             4/2×0.04 = 0.08 mol

Mass of iron produced:

Mass = number of moles × molar mass

Mass = 0.08 mol × 55.85 g/mol

Mass = 4.468 g

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Answer:

Multiply the number of moles in the product by the molecular weight of the product to determine the theoretical yield.

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So multiply,..

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This is the correct way to calculate the theoretical yield

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