2015 AP Chemistry free response 2a (part 1 of 2) | Chemistry | Khan Academy | Summary and Q&A

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April 21, 2016
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2015 AP Chemistry free response 2a (part 1 of 2) | Chemistry | Khan Academy

TL;DR

The content explains the process of dehydrating ethanol to produce ethene and provides calculations to determine the number of moles of ethene produced.

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Questions & Answers

Q: How is ethene produced from the dehydration of ethanol?

Ethene is produced from the dehydration of ethanol through a chemical reaction in the presence of a solid catalyst. The reaction yields ethene and water.

Q: What is the purpose of the experiment described in the content?

The purpose of the experiment is to determine the number of moles of ethene produced during the dehydration of ethanol. This allows for the calculation of the percent yield of ethene.

Q: How is the partial pressure of ethene calculated?

The partial pressure of ethene can be calculated by subtracting the partial pressure of water from the total pressure. The partial pressure of water is determined by converting the vapor pressure of water from torr to atmospheres.

Q: How is the number of moles of ethene calculated in the experiment?

The number of moles of ethene can be calculated using the Ideal Gas Law equation. By knowing the partial pressure of ethene, volume, gas constant, and temperature, the number of moles can be determined.

Summary & Key Takeaways

  • Ethanol can be dehydrated using a solid catalyst to produce ethene and water.

  • A student conducted an experiment where they added a sample of ethanol to a test tube and heated it until all the ethanol evaporated and gas generation stopped.

  • The volume of gas collected was measured, along with the total pressure and temperature, to calculate the number of moles of ethene produced.

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