Question

For the following reaction, the starting material weighs 3.00 grams and the final product weighs 2.00...

For the following reaction, the starting material weighs 3.00 grams and the final product weighs 2.00 grams. what is the percent yield for this reaction?

Cyclohexanol -----> cyclohexene + h2o

cyclohexanol molar mass: 100 grams

cyclohexene molar mass: 82 grams

Homework Answers

Answer #1

ANSWER:

The given reaction is:

Cyclohexanol Cyclohexene + H2O

Mass of cyclohexanol = 3.00 g

Mass of cyclohexene = 2.00 g

molar mass of cyclohexanol = 100 g

molar mass of cyclohexene = 82 g

Number of moles of reactant (cyclohexanol) = (mass)/(molar mass)

= (3.00)/(100)

= 0.03 moles

For the given reaction, one moles of reactant will give one mole of product. Since, number of moles of reactant is 0.03 moles so, number of moles of product will be 0.03 moles also by the theoritical calculation.

Theoritical mass of product = number of moles x molar mass

= 0.03 moles x 82 g/mol

= 2.46 g

And, given mass of product is 2.00 grams. So,

Percentage yield = (given mass x 100)/(theoritical mas)

= (2.00 g x 100)/(2.46 g)

= 81.30 %

Hence, the percent yield for this reaction is 81.30 %.

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