Reaction of bleach and acetic acid to create HOCl (hypochlorous acid) which is a

ID: 534114 • Letter: R

Question

Reaction of bleach and acetic acid to create HOCl (hypochlorous acid) which is a oxidizing reagent. The HOCl then reacts with isoborneol (secondary alcohol) to create camphor! This is the end of the reaction/ experiment where the product is camphor. I need help calculating the theoretical yield of this reaction in lab class. The TA said to google and find the ratio of Isoborneol to Camphor producted but I cant find it anywhere.

My actual yield was 0.99 grams of camphor and i need to find the percent yield but im missing theoretical yield. How do you find the theoretical yield for this reaction?

Explanation / Answer

Ans. Camphor synthesis:

Net Reaction: Isoborneol ------(NaOCl / CH3COOH)--------> Camphor

Stoichiometry: 1 mol Isoborneol forms 1 mol camphor.

Calculation of Theoretical Yield : To calculate the theoretical yield, the amount of Isoborneol taken must be known. Since it is NOT provided in the question, I proceed with a hypothetical value.

Amount of Isoborneol (C10H18O) taken = 2.5 g

Moles of Isoborneol = Mass / Molar mass = 2.5 g / (154.25 g mol-1) = 0.0162 mol

See the stoichiometry: 1 mol Isoborneol forms 1 mol camphor. So, theoretical moles of camphor produced from 2.5 g Isoborneol (= 0.0162 mol) is equal to 0.0162 mol.

So,

Theoretical moles of Camphor produced = 0.0162 mol

Theoretical mass of camphor produced = Moles x Molar mass

= 0.0162 mol x (152.23 g mol-1)

= 2.47 g

Therefore, theoretical yield = 2.47 g

Note: Theoretical yield depends on the “amount of Isoborneol taken for reaction”. Calculate your theoretical yield using the mass of Isoborneol you took for the reaction.

## Calculating % Yield

% yield = (Actual yield/ Theoretical yield) x 100

Ref: Stoichiometry of reaction-

http://www.brynmawr.edu/chemistry/Chem/mnerzsto/oxidation_isoboreol.pdf