What mass of sulfuric acid can be obtained from 1 ton of pyrite with a yield of 90%?

Let’s execute the solution:
1. Let’s write down the equation, select the coefficients:
4FeS2 + 15O2 + 8H2O = 2Fe2O3 + 8H2SO3 – burning of sulfur pyrite (pyrite), sulfuric acid, iron oxide are formed;
2. Let’s calculate the molar masses of substances:
M (FeS2) = 120 g / mol;
M (H2SO4) = 98 g / mol.
3. Determine the amount of moles of pyrite, sulfuric acid:
Y (FeS2) = m / M = 1000/120 = 8.33 mol;
8.33 mol (FeS2) – X mol (H2SO4);
– 4 mol – 8 mol from here, X mol (H2SO4) = 8.33 * 8/4 = 16.6 mol.
We find the theoretical mass of sulfuric acid:
m (H2SO4) = Y * M = 16.6 * 98 = 162.68 g.
The practical mass is calculated taking into account the product yield:
W = m (practical) / m (theoretical) * 100;
m (practical) = 0.90 * 162.68 = 146.41 g.
Answer: the mass of sulfuric acid is 146.41 g.