1. Ammonium nitrate decomposes into nitrous oxide and water according to the following balanced
NH4NO3 → N2O + 2H2O
(I) Assuming that all of the molecules decomposed and based on this decomposition reaction, fill in the blanks of the following statements:
a) One molecule of NH4NO3 produces __molecule(s) of N2O and
___ molecules(s) of water.
b) One mole of NH4NO3 produces ___ mole(s) of N2O and
___ mole(s) of water.
c) Ten molecules of NH4NO3 would produce___ molecules of N2O
and ___ molecule(s) of water.
d) 2.5 moles of NH4NO3 produces ___ mole(s) of N2O and
and ___ mole(s) of water.
(II) Determine the mass of water and nitrous oxide that can be produced from 50 g of ammonium nitrate. Assume 100% efficiency.
2. A chemist makes nitroglycerine, C3H5(NO3)3, from glycerol, C3H5(OH)3, and nitric acid according to the following balanced equation:
C3H5(OH)3 + 3HNO3 → C3H5(NO3)3 + 3H2O
a) In one experiment, 4.1 g of glycerol and 13.5 g of nitric acid produced 5.5 g of nitroglycerine. What was the percent yield of nitroglycerine?
b) Offer a brief explanation as to why this reaction did not yield 100% products.
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