i never understood this problem? can someone plss help..
A student reacts benzene,C6H6. with bromine. Br2. in an attempt to prepare bromobenzene.
C6HSBr :
C6H6 + Br2·---·-> C6H5Br + HBr
(a) What is the theoretical yield of bromobenzene in this reaction when 60.0 g of benzene reacts with 60.0 g Br2?
b) If the actual yield of bromobenzene was 56.7 g, what was the percentage yield?
I mole of benzene reacts with one mole of Br2
This reaction takes place in the presence of catalyst AlBr3
60.0g of benzene ---> moles of benzene---> moles of bromobenzene
60.0g of Br2 ---> moles of Br2---> moles of bromobenzene
the one which gives the least amount of the product will be the limiting reactant
here Br2 is the limiting reactant
convert the moles of bromobenzene obtained from Bromine into grams of bromobenzene
this will be give the theoretical yield
now to take out % yield
= actual yield x 100% / theoretical yield