Consider the reaction of cyclohexanol and an acid catalyst to obtain cyclohexene.

Cyclohexanol (100.16 g/mol) --> Cyclohexene (82.14 g/mol)

A reaction was performed in which 3.1 g of cyclohexanol was reacted with an acid catalyst to obtain 2.2 g of cyclohexene. Calculate the percent yield for this reaction (in %).

[tex]\text{ Moles of Cyclohexanol }=\frac{\text{ Mass of Cyclohexanol }}{\text{ Molar mass of Cyclohexanol }}=\frac{3.1g}{100.16g/mole}=0.03095moles[/tex]

Now we have to calculate the moles of Cyclohexene.

The balanced chemical reaction is,

[tex]Cyclohexanol\rightarrow Cyclohexene[/tex]

From the reaction, we conclude that

As, 1 mole of Cyclohexanol react to give 1 mole of Cyclohexene

So, 0.03095 mole of Cyclohexanol react to give 0.03095 mole of Cyclohexene

Now we have to calculate the mass of Cyclohexene.

[tex]\text{ Mass of Cyclohexene}=\text{ Moles of Cyclohexene}\times \text{ Molar mass of Cyclohexene}[/tex]

[tex]\text{ Mass of Cyclohexene}=(0.03095moles)\times (82.14g/mole)=2.542g[/tex]

Theoretical yield of Cyclohexene = 2.542 g

Experimental yield of Cyclohexene = 2.2 g

Now we have to calculate the percent yield of reaction.

[tex]\% \text{ yield of reaction}=\frac{\text{ Experimental yield of Cyclohexene}}{\text{ Theretical yield of Cyclohexene}}\times 100[/tex]

[tex]\% \text{ yield of reaction}=\frac{2.2g}{2.542g}\times 100=86.5\%[/tex]

Therefore, the percent yield of the reaction is, 86.5 %