Question

4fe(s)+3o2(g)→2fe2o3(s) how many grams of Fe2O3 are produced when 12.0 of iron rusts

Answer 1

Answer:

Mass = 10.1 g

Explanation:

Given data:

Mass of Fe₂O₃ produced = ?

Mass of iron rust = 12.0 g

Solution:

Chemical equation:

4Fe + 3O₂    →  2Fe₂O₃

Number of moles of iron:

Number of moles = mass/ molar mass

Number of moles = 12.0 g/ 55.85 g/mol

Number of moles = 0.215 mol

Now we will compare the moles of iron and Fe₂O₃ .

                     Fe            :          Fe₂O₃

                      4             :              2

                       0.215     :          2/4×0.125 = 0.063 mol

Mass of  Fe₂O₃ :

Mass = number of moles × molar mass

Mass = 0.063 mol × 159.7 g/mol

Mass = 10.1 g

Answer 2

The mass of  Fe₂O₃ is 10.1 grams.

Given:

Mass of iron rust = 12.0 g

To find:

Mass of Fe₂O₃ produced = ?

Balanced Chemical reaction:

4Fe + 3O₂    →  2Fe₂O₃

Calculation for number of moles of iron:

Number of moles = mass/ molar mass

Number of moles = 12.0 g/ 55.85 g/mol

Number of moles = 0.215 mol

According to mole-ratio concept:

Fe          :          Fe₂O₃

4            :              2

0.215     :          2/4×0.125 = 0.063 mol

Calculation for mass of Fe₂O₃ :

Mass = number of moles × molar mass

Mass = 0.063 mol × 159.7 g/mol

Mass = 10.1 g

Thus,  10.1 g of Fe₂O₃ are produced.

Find more information Number of moles here:

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