Answer :
The theoretical yield of cyclohexene is 23.5 g and the percentage yield is 51.06%, the complete reaction is: C₆H₁₀ + Br₂ → C₆H₁₀Br₂, and the two applications of cyclohexene are: Production of nylon, and solvent.
To calculate the theoretical yield of cyclohexene: Convert the volume of cyclohexanol used to mass, using its density (0.962 g/mL): 20.0 mL x 0.962 g/mL = 19.24 g
Calculate the number of moles of cyclohexanol used: 19.24 g / 82.19 g/mol = 0.234 mol
Use the stoichiometry of the reaction to determine the number of moles of cyclohexene that should be produced, assuming 100% yield. The balanced equation is: Cyclohexanol (C₆H₁₁OH) → Cyclohexene (C₆H₁₀) + H₂O
For every 1 mole of cyclohexanol used, 1 mole of cyclohexene should be produced.
Calculate the theoretical yield of cyclohexene in grams: 0.234 mol x 100.2 g/mol = 23.5 g
To calculate the percentage yield of cyclohexene: Divide the actual yield of cyclohexene obtained (12.0 g) by the theoretical yield (23.5 g), and multiply by 100 to get the percentage: (12.0 g / 23.5 g) x 100 = 51.06%
The reaction for bromine test between cyclohexene and bromine is: C₆H₁₀ + Br₂ → C₆H₁₀Br₂
This reaction results in the addition of the bromine molecule across the double bond in cyclohexene, forming a dibrominated product.
Two applications of cyclohexene are:
Production of nylon: Cyclohexene is used in the production of adipic acid, which is a key component in the production of nylon fibers and plastics.
Solvent: Cyclohexene is used as a solvent in various chemical reactions and in the manufacturing of some pharmaceuticals.
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