1. Consider this reaction: 10.5 mL of cyclohexanol and 5 mL of 9 M sulfuric acid

Question

1. Consider this reaction: 10.5 mL of cyclohexanol and 5 mL of 9 M sulfuric acid react to form cyclohexene. a. In this experiment, sulfuric acid is a catalyst. As such, why can it not be the limiting reagent? b. Calculate the number of moles of cyclohexonol in 10.5 mL. Show work. c. What would be the theoretical yield (in grams) of cyclohexene in this reaction? 2. If 6.2 g of cyclohexene was obtained from the reaction above, in pure form, what is the percent yield? Show work. 3. If the percent yield was 68% and you obtained 1.34 g, what was your theoretical yield?

Explanation / Answer

1. In case of dehdyration of cyclohexanol we are taking excess of sulphuric acid so we can not take it as limiting reagent.

b Density of cyclohexanol = 0.96 g/ mL

volume given = 10.5 mL

so mass of cyclohexanol = 10.08 g

Molecular wt = 100g /mole

So mole= mass / mol wt = 10.8 / 100 = 0.1008 moles

c. Theoretical yield will be 0.1008 moles, as one mole of cyclohexanol is giving one mole of hexene

now mol wt of cyclohexene = 82 g / mole

So mass = 82 X 0.1008 = 8.265 g ( theoretical yield)

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