Asked by Dania sarash
If I have cyclohexene in a hydroboration-oxidation reaction to form cyclohexanol how can I find percentage yield?
I have NaBH4 (0.0610) and boron triflouride etherate (0.0162) and they are in a 4 to 3 ratio to form b2h6 (diborane) so diborane number of moles is based on boron triflouride etherate as its the limiting reagent so then I plug in to the overall reaction 3cyclohexene (0.0594mol) + b2h6 to form 3cyclohexanol. so according to the overall reaction b2h6 is the limiting reagent so will use that to form cyclohexanol using ratio 1:3?
I have NaBH4 (0.0610) and boron triflouride etherate (0.0162) and they are in a 4 to 3 ratio to form b2h6 (diborane) so diborane number of moles is based on boron triflouride etherate as its the limiting reagent so then I plug in to the overall reaction 3cyclohexene (0.0594mol) + b2h6 to form 3cyclohexanol. so according to the overall reaction b2h6 is the limiting reagent so will use that to form cyclohexanol using ratio 1:3?
Answers
Answered by
DrBob222
% yield = (actual yield/theoretical yield)*100 = ?
The actual yield is what the problem tells you the reaction produces. The theoretical yield is what you calculate is formed from the stoichiometry.
The actual yield is what the problem tells you the reaction produces. The theoretical yield is what you calculate is formed from the stoichiometry.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.