Answered

At Westonci.ca, we connect you with the answers you need, thanks to our active and informed community. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals. Experience the ease of finding precise answers to your questions from a knowledgeable community of experts.

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?

Sagot :

Nepalieducation

Answer:

952.2g SO3

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.

Thank you for trusting us with your questions. We're here to help you find accurate answers quickly and efficiently. Thank you for choosing our platform. We're dedicated to providing the best answers for all your questions. Visit us again. Keep exploring Westonci.ca for more insightful answers to your questions. We're here to help.