Nitrobenzene, C6H5NO2, is prepared from benzene, C6H6, and nitric acid, HNO3. The other product of the reaction is water. When 22.4 g of benzene is reacted with an excess of nitric acid, 31.6 g of nitrobenzene is produced. What is the percent yield for this reaction?

Answer 1

1. Write and balanced the equation.
2. Convert 22.4 g benzene to mols. mols = grams/molar mass = ?
3. Using the coefficients in the balanced equation, convert mols benzene to mols nitrobenzene. This is the theoretical (TY) for the reaction.
4. The actual yield (AY) is 31.6
5. %yield = (AY/TY)*100 = ?

Answer 2

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Answer 3

Consider the preparation of nitrobenzene, C6H5NO2, by the reaction of a limited amount of benzene,
C6H6, with excess nitric acid, HNO3. The balanced equation for the reaction may be written as
C6H6 + HNO3 → C6H5NO2 + H2O
A 15.6-g sample of C6H6 is mixed with excess HNO3. We isolate 18.0 g of C6H5NO2. What is the
percent yield of C6H5NO2 in this reaction?

Answer 4

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