Question

How would I calculate theoretical yield of a reaction involving using .8mL of sulfuric acid as a catalyst and 2mL of water in an acid-catalyzed hydration reaction of 0.6mL of the alkene 1-hexene. 3mL of Ether was also used to dilute the organic layer but was theoretically mostly all evaporated out with a stream of nitrogen. I need to know how much 2-hexanol and 1-hexanol major and minor products would theoretically be produced.

Answer 1

Volume of 1- hexene used = 0.6 ml

Density of 1 - hexene = 0.673 g/ ml

Mass of 1- hexene used = volume × density = 0.6 ml × 0.673 g/ ml = 0.404 g

Moles of 1- hexene used = mass / molar mass = 0.404 g / (84 g/mole) = 0.0048 mol

Total Moles of product produced = 0.0048 mol (theoretical yield)

Product is a mixture of 1-hexanol and 2- hexanol . Both have the molar mass of 102 g/ mol

So; theoretical yield of products (total as a mixture of the two products) = 0.0048 mol × 102 g/ mol = 0.49 g

Its not possible to tell the exact theoretical yield for each product if you don't know the ratio at which they are formed.