Question

Suppose you are performing a hydroboration oxidation of 1-hexene to form 1-hexanol. Your reaction includes 0.82 mL of 1-hexene, which has a density of 0.673 g/mL, 1.80 mL of 1.00 M borane in THF, and 1.31 mL of 30.0% m/v hydrogen peroxide. What is the theoretical yield of 1-hexanol (in g) for the reaction

Answer 1

From the stoichiometry of the reaction 0.18 g of 1-hexanol is formed.

What is theoretical yield?

The theoretical yield of a compound is its yield based on the stoichiometry of the reaction.

We must now obtain the number of moles of each reactant:

For hexane;

Mass of hexane = Density × volume = 0.82 mL × 0.673 g/mL = 0.55 g

Number of moles = 0.55 g/84 g/mol = 0.0065 moles

For borane;

Number of moles = concentration × volume = 1.00 M × 1.80/1000 L = 0.0018 moles

Since the reaction is 1:1, borane is the limiting reactant, hence;

Number of moles of 1-hexanol = 0.0018 moles × 102 g/mol = 0.18 g

Learn more about stoichiometry: brainly.com/question/9743981