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- Title: Cyclohexene
- Type: Notes
- School: McGill
- Course: CHEM 222
- Term: Spring
Coursehero >> Canada >> McGill >> CHEM 222
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Path: SFASU >> PSY >> 153 Fall, 2005
Path: SFASU >> PSY >> 153 Fall, 2005
Path: SFASU >> PSY >> 153 Fall, 2005
Path: SFASU >> PSY >> 153 Fall, 2005
Path: SFASU >> PSY >> 153 Fall, 2005
Path: SFASU >> PSY >> 153 Fall, 2005
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Path: Texas >> M >> 362k Spring, 2008
Path: Texas >> M >> 362k Spring, 2008
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Path: Texas >> M >> 362k Spring, 2008
Path: Texas >> M >> 362k Spring, 2008
Path: Texas >> M >> 362k Spring, 2008
Path: Texas >> M >> 362k Spring, 2008
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The Intro: purpose of this experiment is to understand the techniques used to synthesize and extract an alkene from an alcohol, which in this experiment are cyclohexene and cyclohexanol. Reactions: The elimination reaction that occurs in the formation of cyclohexene is E1, occurring in 3 steps. First, the alcohol group of cyclohexanol is protonated using phosphoric acid, a strong acid. Secondly, the resulting positively charged H20 group is weakened and breaks off of cyclohexanol, resulting in a carbocation. Thirdly, a proton is expelled from the molecule, resulting in the formation of cyclohexene and a hydronium ion. Discussions: One important thing to keep in mind when performing an elimination reaction is that these reactions are reversible. As the fueling process of this reaction is protonation, which is completely reversible, one must remember that there is an equilibrium between the formation of products and the reformation of reactants. The significance of this is best said by le chatelier's principle in that "when you distill an alkene and remove the products from the solution, you push the equilibrium towards the formation of more products." This motif is central to understanding the procedure and success of this experiment, this as experiment involved two distillations. As stated above, when we distilled our solution, we removed the cyclohexene product, pushing the equilibrium of the remaining solution towards the formation of more products. The reason it is known that cyclohexene will be distilled, and not cyclohexanol is from the molecular structure of the two molecules. As cyclohexanol has an OH group, it can perform hydrogen bonds with its surroundings and itself, which causes its boiling point to increase, whereas cyclohexene cannot perform hydrogen bonding, and thus has a lower boiling point. In the VPC of our final solution there were three distinct curves, corresponding to the product (cyclohexene), reactant (cyclohexanol), and elimination (xylene) content of the solution. But, being foolish, I neglected to take the final weight of the solution, and can thus not effectively analyze the data. Instead are the attached calculations of our VPC analysis using a friend's combined weight. Our VPC did however tell us the percentage of the different contents of our solution, which were relatively off. This is due to the excess xylene that was distilled along with the cyclohexene. www.chemguide.co.uk/physical/equilibria/lechatelier.html
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