Determine the volume of hydrogen consumed for the reduction of 16.8 g of iron from iron oxide (III).

Let’s execute the solution:

In accordance with the condition of the problem, we compose the equation of the process:
Fe2O3 + 3H2 = 2Fe + 3H2O – OBP, iron is released;

Let’s make calculations using the formulas of substances:
M (Fe2O3) = 159.6 g / mol;

M (H2) = 2 g / mol;

Y (Fe2O3) = m / M = 16.8 / 159.6 = 0.1 mol.

Proportion:
0.1 mol (Fe2O3) – X mol (H2);

-1 mol -3 mol from here, X mol (H2) = 0.1 * 3/1 = 0.3 mol.

We find the volume of H2:
V (H2) = 0.3 * 22.4 = 6.72 L

Answer: you need hydrogen with a volume of 6.72 liters