For the reaction: 4Fe+3O2= 2Fe2O3 if 100g of Fe are used how much of O2 is used

Mass = 42.88 g

Explanation:

Given data:

Mass of iron = 100 g

Mass of O₂ = ?

Solution:

Chemical equation:

4Fe + 3O₂       →    2Fe₂O₃

Number of moles of Iron:

Number of moles = mass/molar mass

Number of moles = 100 g/ 55.85 g/mol

Number of moles = 1.79 mol

Now we will compare the  moles iron with oxygen.

                               Fe          :              O₂

                                 4            :               3

                                 1.79        :           3/4×1.79 = 1.34 mol

Mass of oxygen used:

Mass = number of moles × molar mass

Mass = 1.34 mol × 32 g/mol

Mass = 42.88 g

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.