Question

Calculate theoritical percent yield of cyclohexanone from cyclohexanol in a hypochlorite oxidation reaction with:

a. 0.150 g cyclohexanol
b. 0.12g acetic acid
c. 2.5 mL of a 5.25% sodium hypochlorite solution

Answer 1

To calculate the theoretical percent yield of cyclohexanone, one needs to determine the molar mass of both cyclohexanol and cyclohexanone, calculate the moles of cyclohexanol, use stoichiometry with the balanced equation to find the theoretical yield in moles and grams, and then calculate the percent yield from the ratio of actual yield to theoretical yield.

Step-by-step explanation:

To calculate the theoretical percent yield of cyclohexanone from cyclohexanol in a hypochlorite oxidation reaction, follow these steps:

1. Determine the molar mass of cyclohexanol and cyclohexanone.
2. Calculate the moles of cyclohexanol used based on its mass (0.150 g).
3. Write the balanced chemical equation for the oxidation reaction.
4. Use stoichiometry to find the theoretical yield (moles) of cyclohexanone produced from the cyclohexanol.
5. Convert this to grams using the molar mass of cyclohexanone.
6. Divide the actual yield (if given) by the theoretical yield and multiply by 100 to get the percent yield.

Note that the masses of acetic acid and sodium hypochlorite solution provided will not directly affect the percent yield calculation unless we are considering their role as limiting reagents or in determining excess reactants, which requires additional information about the reaction stoichiometry.