Find the mass of sulfuric acid obtained from 1 ton of perite containing 30% impurities. If the yield is 80%.

| September 7, 2021 | education

Let’s find the mass of pyrite without impurities.

100% – 30% = 70%.

1000 kg – 100%,

X kg – 70%,

X = (1000 kg × 70%): 100% = 700 kg.

Let’s find the amount of pyrite substance.

M (FeS2) = 184 kg / kmol.

n = m: M.

n = 700 kg: 184 kg / kmol = 3.8 kmol.

Let’s compose the reaction equation. Let’s find the quantitative ratios of substances.

(1) 4FeS2 + 11О2 = 2 Fe2O3 + 8SO2.

(2) 2SO2 + O2 = 2SO3.

(3) SO3 + H2O = H2SO4.

According to the reaction equation (1), there is 8 mol of SO2 per 4 mol of FeS2. Substances are in quantitative ratios 4: 8 = 1: 2. The amount of SO2 is 2 times more than FeS2.

n (SO2) = 2 n (FeS2) = 3.8 × 2 = 7.6 kmol.

n (SO2) = n (SO3) = 7.6 kmol.

n (SO3) = n (H2SO4) = 7.6 kmol.

Let’s find the mass of Н2SO4.

m = n × M,

M (H2SO4) = 98 kg / kmol.

m = 7.6 kmol × 98 kg / kmol = 744.8 kg.

744.8 kg -100%,

X – 80%,

X = (744.8 kg × 80%): 100% = 595.84 kg.

Answer: 595, 84 kg.



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