In the presence of an acid catalyst, cyclohexanol (100.16 g/mol) is dehydrated to give cyclohexene (82.14 g/mol) and water. Reaction scheme illustrating the dehydration of cyclohexanol in the prescence of acid catalyst to cylcohexene and water. A dehydration reaction starting with 4.1 g cyclohexanol produces 3.0 g cyclohexene. Calculate the percent yield for this reaction. Report your answer with two significant figures.

88%

Explanation:

Step 1: Write the balanced equation

C₆H₁₁OH ⇒ C₆H₁₀ + H₂O

Step 2: Calculate the moles corresponding to 4.1 g of C₆H₁₁OH

The molar mass of C₆H₁₁OH is 100.16 g/mol.

4.1 g × 1 mol/100.16 g = 0.041 mol

Step 3: Calculate the theoretical yield, in moles, of C₆H₁₀

The molar ratio of C₆H₁₁OH to C₆H₁₀ is 1:1. The theoretical yield of C₆H₁₀, in moles, is 1/1 × 0.041 mol = 0.041 mol.

Step 4: Calculate the mass corresponding to 0.041 moles of C₆H₁₀

The molar mass of C₆H₁₀ is 82.14 g/mol.

0.041 mol × 82.14 g/mol = 3.4 g

Step 5: Calculate the percent yield of C₆H₁₀

We will use the following expression.

percent yield = experimental yield/theoretical yield × 100%

percent yield = 3.0 g/3.4 g × 100% = 88%

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