1.        Ammonium nitrate decomposes into nitrous oxide and water according to  the following balanced

chemical equation:

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.