To determine the mass of iron oxide produced when 100 g of medium fine steel wool with a strand diameter of 0.002 inch is burned, we need to calculate the percentage of iron in the steel wool, and then use stoichiometry to determine the mass of iron oxide produced.
Assuming that the steel wool is made entirely of iron, the percentage of iron in the steel wool is 100%. We can then calculate the mass of iron in the steel wool by multiplying the total mass by the percentage of iron:
Mass of iron = 100 g x 100% = 100 g
Next, we need to use the balanced chemical equation for the combustion of iron:
4Fe + 3O2 → 2Fe2O3
From the equation, we can see that 4 moles of iron react with 3 moles of oxygen to produce 2 moles of iron oxide.
The molar mass of iron is 55.845 g/mol, and the molar mass of iron oxide (Fe2O3) is 159.69 g/mol.
Using the mole ratio from the balanced chemical equation, we can calculate the moles of iron oxide produced:
Moles of Fe2O3 = (2/4) x (100 g / 55.845 g/mol) = 0.714 mol
Finally, we can use the molar mass of iron oxide to calculate the mass of iron oxide produced:
Mass of Fe2O3 = 0.714 mol x 159.69 g/mol = 113.97 g
Therefore, when 100 g of medium fine steel wool with a strand diameter of 0.002 inch is burned, we would expect to produce 113.97 g of iron oxide