anonymous
  • anonymous
A chemist reacted 300 g of 1-butene with excess Br2 (in CCl4) at 25 8C. He isolated 418 g of 1,2-dibromobutane. What is the percent yield?
Organic
jamiebookeater
  • jamiebookeater
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matt101
  • matt101
Br2 is added across the double bond in 1-butene to form a dihalide. The balanced reaction would be: \[C_{4}H_{8}+Br_{2} \rightarrow C_{4}H_{8}Br_{2}\] We have 300 g of 1-butene, which is 300 g / 56 g/mol = 5.36 mol. According to the reaction, this means we should also get 5.36 mol of 1,2-dibromobutane, which has a mass of 5.36 mol x 216 g/mol = 1158 g. The formula for percent yield is: \[percent \space yield = \frac{mass \space of \space actual \space yield}{mass \space of \space theoretical \space yield} \times 100\] So let's just plug our numbers in to find the answer: \[percent \space yield = \frac{418 \space g}{1158 \space g} \times 100 =36.1\] The percent yield for this reaction is 36.1%.

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