How many grams of oxygen are needed to react with 350g of iron to produce 500 g of Fe2O3
To find the amount of oxygen needed to react with 350g of iron to produce 500g of Fe2O3, we first need to determine the molar mass of iron (Fe) and Fe2O3.
The molar mass of Fe is approximately 56 g/mol.
The molar mass of Fe2O3 can be calculated as follows:
Fe = 56 g/mol x 2 = 112 g/mol
O = 16 g/mol x 3 = 48 g/mol
Fe2O3 = 112 + 48 = 160 g/mol
Next, we need to determine the number of moles of Fe and Fe2O3 in the given masses of iron and Fe2O3:
Number of moles of Fe = 350g / 56 g/mol = 6.25 mol
Number of moles of Fe2O3 = 500g / 160 g/mol = 3.125 mol
From the balanced chemical equation for the reaction of iron with oxygen to form Fe2O3:
4Fe + 3O2 → 2Fe2O3
We can see that 4 moles of Fe react with 3 moles of O2 to produce 2 moles of Fe2O3.
To find the number of moles of O2 required to react with 6.25 moles of Fe to produce 3.125 moles of Fe2O3, we use the mole ratio of O2 to Fe in the balanced chemical equation:
(3/4) x 6.25 mol = 4.69 mol
Finally, we convert the number of moles of O2 to grams:
4.69 mol x 32 g/mol = 150.08 g
So, 150.08 grams of oxygen are needed to react with 350g of iron to produce 500g of Fe2O3.