Question

A chemist burns 650.0 g of C4H8S2 in excess oxygen, according the following balanced chemical reaction:

C4H8S2+ 902 -> 4CO2 + 4H2O +2S03
If the chemist has 92.2% yield, how many grams of SO3 were produced?

Answer 1

952.2g SO3

Step-by-step explanation:

Molar mass of C4H8S2 is 120.2363 g/mol

Mol in 750.0g = 750.0/120.2363 = 6.238 mol

1mol C4H8S2 produces 2 mol SO3

6.238 mol will produce 2×6.238 = 12.476 mol SO3

Molar mass SO3 = 32+3×16 = 80.0g/mol

Theoretical yield = 12.476×80.0 = 998.08g

The actual yield is 95.4%

Actual mass-produced = 95.4/100×998.08 = 952.2g SO3 produced

Hope it will help you.