Calculate the mass of iron formed when it is reduced from iron (III) oxide weighing 80 g, if the mass fraction
Calculate the mass of iron formed when it is reduced from iron (III) oxide weighing 80 g, if the mass fraction of the product yield is 80%
1. The reduction of iron from oxide occurs in accordance with the reaction:
Fe2O3 + 3H2 = 2Fe + 3H2O;
2.Considering the product yield, let us establish the practical mass of the reacted oxide:
mpr (Fe2O3) = ν * mtheor (Fe2O3) = 0.8 * 80 = 64 g;
3. Find the chemical amount of iron oxide:
n (Fe2O3) = mpr (Fe2O3): M (Fe2O3);
M (Fe2O3) = 2 * 56 + 3 * 16 = 160 g / mol;
n (Fe2O3) = 64: 160 = 0.4 mol;
4. The amount of iron is twice the amount of oxide, since two units of iron are released from one oxide molecule:
n (Fe) = n (Fe2O3) * 2 = 0.4 * 2 = 0.8 mol;
5. Let’s calculate the mass of iron:
m (Fe) = n (Fe) * M (Fe) = 0.8 * 56 = 44.8 g.
Answer: 44.8 g.