In the presence of an acid catalyst, cyclohexanol (100.16 g/mol) is dehydrated to give cyclohexane (82.14 g/mol) and water. A dehydration reaction starting with 3.3 g cyclohexanol produces 2.4 g cyclohexene. Calculate the theoretical yield for this reaction. Report your answer with two significant figures.

A theoretical yield is the amount of products created by a chemical reaction, provided none of the reactants were wasted and the reaction was fully completed.

Let's write out the balanced chemical equation for the reaction;

Cyclohexanol --> Cyclohexane + Water

HOCH(CH2)5 --> C6H10 + H2O

Step 1: Determine the number of moles of each reactant

Number of moles = Mass/ molar mass = 3.3 / 100.16 = 0.03295 mol

From the equation; 1 mole of cyclohexanol produces 1 mol of cyclohexene.

This means 0.03295 mol of cyclohexanol produces 0.03295 mol of cyclohexene.

Mass of cyclohexene produced; Mass = Number of moles * Molar mass = 0.03295 * 82.14 = 2.71g

pstnonsonjoku pstnonsonjoku · Answer 2 · 2022-01-27T13:58:06+01:00

The theoretical yield of the reaction is 2.7 g.

We know that the reaction is 1:1 hence;

Number of moles of cyclohexanol = 3.3 g/100 g/mol = 0.033 moles

Number of moles of cyclohexene = 2.4 g /82 g/mol = 0.029 moles

Hence;

Theoretical yield of cyclohexene = 0.033 moles or 2.7 g

Actual yield of cyclohexene = 0.029 moles

Percentage yield = actual yield/theoretical yield × 100/1

Percentage yield = 0.029 moles/0.033 moles × 100/1 = 88%

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