Calculate the volume of CO required to completely reduce 10 g of Fe2O3

1. Let’s write down the reaction equation:
Fe2O3 + 3CO = 3CO2 + 2Fe – redox reaction, iron and carbon dioxide are released;
2. Determine the molecular weights of the reactants:
M (Fe2O3) = 2 * 55.8 + 16 * 3 = 159.6 g / mol;
M (CO) = 12 + 16 = 28 g / mol;
3. Determine the amount of moles of iron oxide by the formula:
Y (Fe2O3) = m / M = 10 / 159.6 = 0.06 mol;
4. Let’s make the proportion using the given reaction equations:
0.06 mol (Fe2O3) – X mol (CO);
-1 mol – 3 mol from here, X mol (CO) = 0.06 * 3/1 = 0.18 mol;
5. Let’s calculate the volume of carbon monoxide (2):
V (CO) = 0.18 * 22.4 = 4 liters.
Answer: to carry out the reaction, carbon monoxide in a volume of 4 liters is required.