Original post by xoxo123j
A student predicted that the yield of this reaction would be greater than 75%. In an experiment,2.00g of ethane was added to an excess of hydrogen bromide and 6.00g of product was obtained.Was the student correct? Justify your answer with a calculation using these data
Equation for the reaction is c2h4 +HBr --> C2H5Br
So one mole of ethane gives one mole c2h5br
Calculate moles ethane in 2.0g
Deduce no of moles of product you should form, hence mass of product that should form
% yield=actual mass/expected mass x 100
See attachment for more details
Original post by Davies Chemistry
Equation for the reaction is c2h4 +HBr --> C2H5Br
So one mole of ethane gives one mole c2h5br
Calculate moles ethane in 2.0g
Deduce no of moles of product you should form, hence mass of product that should form
% yield=actual mass/expected mass x 100
See attachment for more details
So one mole of ethane gives one mole c2h5br
Calculate moles ethane in 2.0g
Deduce no of moles of product you should form, hence mass of product that should form
% yield=actual mass/expected mass x 100
See attachment for more details
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(edited 3 years ago)
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