When a chemist treated 28 g of C₄H₈ witH₄8 grams of Cl₂, she isolated 51 g of C₄H₈Cl₂ in pure form. No other products were formed in this reaction. What was the % yield?

Question

Quizplus · Accepted Answer

To find the % yield, we need to first calculate the theoretical yield and then divide the actual yield by the theoretical yield and multiply by 100%. First, we need to determine the limiting reagent. To do this, we can use the mole ratio from the balanced chemical equation: C₄H₈ + 2Cl₂ -> C₄H₈Cl₂ Moles of C₄H₈ = 28 g / (32.06 g/mol) = 0.873 mol Moles of Cl₂ = 14.08 g / (70.906 g/mol) = 0.198 mol The mole ratio of C₄H₈ to Cl₂ is 1:2, so Cl₂ is the limiting reagent. Theoretical yield = (0.198 mol Cl₂) x (1 mol C₄H₈Cl₂ / 2 mol Cl₂) x (278.28 g/mol) = 21.8 g % yield = (51 g / 21.8 g) x 100% = 233.9% However, the % yield cannot be greater than 100%, so the answer is D) 80%.

When a Chemist Treated 28 G of C4H8 WitH48 Grams

When a Chemist Treated 28 G of C₄H₈ WitH₄8 Grams