2) (2 pts) The formation of cyclohexene from cyclohexanol is shown below: OH H3PO4 cyclohexanol Density = 0.96 g/mL MM 100.16 g/mole cyclohexene Density 0.811 g/mL MM = 82.15 g/mole s with 11.5 mL of cyclohexanol and adds a sufficient amount of phosphoric acid to ne. Determine the A student start carry out the dehydration reaction. She recovers 7.84 mL of cyclohexe following… theoretical yield -% yield [% yield (actual yield / theoretical yield) x 100%) Show your calculations!* Hint:-vol. cyclohexanol → g cyclohexanol → moles cyclohexanol → moles cyclohexene → g cyclohexene -determine actual yield from volume of cyclohexene (vol. cyclohexene → g cyclohexene) theoretical yield amount of product based on cyclohexanol
The Correct Answer and Explanation is :
To calculate the theoretical yield and percentage yield for the dehydration reaction of cyclohexanol to cyclohexene, we will follow these steps:
Step 1: Convert volume of cyclohexanol to mass
The density of cyclohexanol is given as 0.96 g/mL, and we are provided with a volume of 11.5 mL of cyclohexanol.
[
\text{Mass of cyclohexanol} = \text{Density} \times \text{Volume}
]
[
\text{Mass of cyclohexanol} = 0.96 \, \text{g/mL} \times 11.5 \, \text{mL} = 11.04 \, \text{g}
]
Step 2: Convert mass of cyclohexanol to moles
The molecular mass (MM) of cyclohexanol is given as 100.16 g/mole. To find the number of moles of cyclohexanol:
[
\text{Moles of cyclohexanol} = \frac{\text{Mass of cyclohexanol}}{\text{Molar mass of cyclohexanol}}
]
[
\text{Moles of cyclohexanol} = \frac{11.04 \, \text{g}}{100.16 \, \text{g/mole}} = 0.110 \, \text{mol}
]
Step 3: Moles of cyclohexene (theoretical yield)
In this dehydration reaction, one mole of cyclohexanol produces one mole of cyclohexene, so the number of moles of cyclohexene will be the same as the number of moles of cyclohexanol.
[
\text{Moles of cyclohexene} = 0.110 \, \text{mol}
]
Step 4: Convert moles of cyclohexene to grams
The molecular mass (MM) of cyclohexene is given as 82.15 g/mole. Now we can find the theoretical mass of cyclohexene.
[
\text{Mass of cyclohexene (theoretical yield)} = \text{Moles of cyclohexene} \times \text{Molar mass of cyclohexene}
]
[
\text{Mass of cyclohexene} = 0.110 \, \text{mol} \times 82.15 \, \text{g/mole} = 9.04 \, \text{g}
]
Step 5: Convert volume of cyclohexene to mass (actual yield)
The density of cyclohexene is given as 0.811 g/mL, and the actual volume recovered is 7.84 mL.
[
\text{Mass of cyclohexene (actual yield)} = \text{Density} \times \text{Volume}
]
[
\text{Mass of cyclohexene (actual yield)} = 0.811 \, \text{g/mL} \times 7.84 \, \text{mL} = 6.36 \, \text{g}
]
Step 6: Calculate the percentage yield
Now, we can calculate the percentage yield using the formula:
[
\% \, \text{yield} = \left( \frac{\text{Actual yield}}{\text{Theoretical yield}} \right) \times 100
]
[
\% \, \text{yield} = \left( \frac{6.36 \, \text{g}}{9.04 \, \text{g}} \right) \times 100 = 70.4\%
]
Final Answer:
- Theoretical yield: 9.04 g of cyclohexene
- Actual yield: 6.36 g of cyclohexene
- Percentage yield: 70.4%
This calculation tells us how efficient the reaction was in producing cyclohexene. The percentage yield reflects how much cyclohexene was actually obtained compared to the theoretical maximum possible amount based on the starting cyclohexanol.
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