Question

To obtain a high yield of nitroacetanilide, 2 equivalents of the nitronium ion will be reacted with acetanilide in this experiment.

If 1 g of acetanilide (molecular weight of acetanilide is 135.17 g/mol) is used, what amount (in mol) of nitronium ion is required? (2 sig figs)

Using the equation: HNO3 + H2SO4 --> NO2 + HSO4 +H2O

If the molecular weight of nitric acid is 63.01 g/mol and its density is 1.5129 g/mL, what volume (mL) of nitric acid is required?  (1 sig fig)

If the molecular weight of sulfuric acid is 98.08 g/mol and its density is 1.84 g/mL, what volume (mL) of sulfuric acid is required? (1 sig figs)

Answer 1

Mass of acetanilide = 1 gm

Molar mass of acetanilide =  135.17 g/mol

Moles of acetanilide = 1gm / 135.17 g/mol = 0.0073980 Moles

Moles of NO2 required = 0.0073980 Moles x 2 = 0.014796 Moles

Moles of HNO3 required =  0.014796 Moles

Mass of HNO3 = 0.014796 Moles x  63.01 g/mol = 0.932 gm

Volume of HNO3 required = 0.932 gm / 1.5129 gm/ml = 0.616 ml

Moles of H2SO4 required =  0.014796 Moles

Mass of H2SO4 = 0.014796 Moles x  98.08 g/mol = 1.4511 gm

Volume of H2SO4 required = 1.4511 gm / 1.84 gm/ml = 0.788 ml