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

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

passing a magnet thought the

mixture , because iron gets attracted to magnet .