Calculate the mass of iron that can be obtained from 160 g of iron (III) oxide, containing 10%
Calculate the mass of iron that can be obtained from 160 g of iron (III) oxide, containing 10% impurities, when it is reduced with carbon.
1. Let’s find the mass of pure iron oxide without impurities.
100% – 10% = 90%.
160 g – 100%,
X – 90%,
X = (160g × 90%): 100% = 144g.
Find the amount of iron (III) oxide substance by the formula:
n = m: M.
M (Fe2O3) = 56 × 2 + 16 × 3 = 160 g / mol.
n = 144 g: 160 g / mol = 0.9 mol.
We compose the reaction equation. We determine in what quantitative ratios the substances are.
Fe2O3 + 3CO = 2Fe + 3CO2.
There are 2 moles of iron per mole of iron oxide. Substances are in quantitative ratios of 1: 2.
The amount of the iron substance will be 2 times more than the amount of the iron oxide substance.
n (Fe) = 0.9 × 2 = 1.8 mol.
Let’s find the mass of iron by the formula:
m = n × M,
M (Fe) = 56 g / mol.
m = 1.8 mol × 56 g / mol = 100.8 g.
Answer: 100.8g.