Reference no: EM132352417

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 ___ 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.