Nitrobenzene (C6H5NO2)(C6H5NO2) is used in small quantities as a flavoring agent or in perfumes, but it can be toxic in large amounts. It is produced by reaction of benzene (C6H6)(C6H6) with nitric acid:
C6H6(l)+HNO3(aq) → C6H5NO2(l)+H2O(l
The limiting reagent is the reactant that limits the amount of product produced. This is the reactant that produces fewer moles of product when it completely reacts. The reaction involves two reactants, C6H6C6H6 and HNO3HNO3, that react in a 1:1 ratio. You are given the masses of both the reactants, 28.0 gg HNO3HNO3 and 74 gg C6H6C6H6. The molar mass of nitric acid is 63.0 g/molg/mol and that of benzene is 78.1 g/molg/mol.
Once you convert 28.0 gg HNO3HNO3 and 74 gg C6H6C6H6 into the number of moles of each using their molar mass, determine which produces less product. Since the coefficients in the balanced chemical equation are all 1, in this specific case you can directly compare the number of moles of each.
Calculate the theoretical yield of C6H5NO2C6H5NO2 for this reaction.
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