Question

In: Chemistry

Using the following atomic weights and that the density of cyclohexanol is 0.96, what is the...

Using the following atomic weights and that the density of cyclohexanol is 0.96, what is the % yield of a reaction that starts with 6.7 mL of cyclohexanol and ends with 2.3 g of cyclohexene?

C = 12, H = 1, O = 16

Solutions

Expert Solution

Mass of cyclohexanol = volume x density

= 6.7 mL x 0.960 g/mL = 6.432 g

C6H12O ---> C6H10 + H2O

Cyclohexanol = cyclohexene + water

The molecular formula of cyclohexanol = C6H12O

molar mass is found by using the atomic masses of C, H, and O..

(6 x 12.0) + (12 x 1) + (1 x 16.0) = 100 g/mol

The molar mass for the cyclohexene

(6 x 12.0) + (10 x 1) = 82 grams per mole.



From the stoichiometry of the reaction

1 mol of C6H12O produces = 1 mol of C6H10

100 g of C6H12O produces = 82 g of C6H10

6.432 g of C6H12O produces = 82*6.432/100 = 5.274 of C6H10

This is also called the "theoretical yield."

The percent yield = (actual yield/theoretical yield) *100


= (2.3 / 5.274) x 100% = 43.61%


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