Question

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

Answer 1

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%