Question

Reaction: C6H11OH(l) ==> C6H10(l) + H2O(l)
Calculate the mass of cyclohexanol (C6H11OH) needed to produce 45.0g cyclohexene (C6H10) by reaction if the reaction has a 86.2% yield and the cyclohexanol is 92.3% pure.
Usually this problem would be fairly easy, but the purity is throwing me off. How does the purity relate to this question?

Answer 1

After you finish the calculation to find the g cyclohexanol needed with 86.2% yield, that is if the cyclohexanolis 100% pure. Since it is only 92.3% pure, the amount for 100%/0.923 = amount needed for 92.3% purity.

Answer 2

Thank you so much!

Answer 3

You don't need to memorize a new formula for this. Remember what you do for %yield. It is
%yield = (actual amount/theoretical yield)*100
92.3 = actual amount/theoretical yield
theoretical = actual/%yield

Answer 4

When heated with sulfuric or phosphoric acid, cyclohexanol, C6H11OH is converted to cyclohexene, C6H10. The balanced chemical equation for the reaction is shown below. C6H11OH(l) → C6H10 (l) + H2O(l) If the percent yield is 83%, what mass of cyclohexanol must we use to obtain 25 g of cyclohexene?