percentage yield =(actual yield/theoretical yield) ×100/1
chlorine is the limiting reagent hence would be the major determinant of the product
71[Cl2]=2×58.5[NaCl]
200[Cl2]=x[NaCl]
x=(200×58.5×2)/(71)
x=329.58g(theoretical yield of NaCl)
percentage yield = (240/329.58) ×100
percentage yield= 72.8℅
The answer is that the percentage yield is 72.8 % .
Chemical reactions in the real world do not always go exactly as planned on paper.
In the course of an experiment, many things will contribute to the formation of less product than would be predicted.
Besides spills and other experimental errors, there are often losses due to an incomplete reaction, undesirable side reactions, etc.
Chemists need a measurement that indicates how successful a reaction has been. This measurement is called the percent yield.
Percentage yield =(actual yield/theoretical yield) ×100 %
Chlorine is the limiting reagent hence would be the major determinant of the product
Molecular weight of Cl₂ is 71
Molecular weight of NaCl is 58.5
For 1 mole of Cl₂ 2 moles of NaCl is produced
so it is given that Cl₂ is 200 grams
= 200/71
=2.82 moles.
=5.63 moles of NaCl
=5.63* 58.5 grams
=329.58 g of Nacl
So , 329.58g is theoretical yield of NaCl
percentage yield = (240/329.58) ×100
percentage yield= 72.8℅
Therefore the percentage yield = 72.8%
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