The balanced decomposition reaction of ammonium nitrate is as follows:
2NH4NO3(s) 2N2(g) + O2(g) + 4H2O(g)
Mass of NH4NO3 = 84.6 g
Determine the number of moles of NH4NO3 from the given mass and molar mass as follows:
The molar mass of NH4NO3 = 80.043 g/mol
= 84.6 g NH4NO3 x ( 1 mol NH4NO3 / 80.043 g NH4NO3)
= 1.0569 mol NH4NO3
Use the moles of NH4NO3 and the mole ratio from the balanced chemical reaction and determine the number of moles of N2, O2, and H2O as follows:
= 1.0569 mol NH4NO3 x ( 2 mol N2 / 2 mol NH4NO3)
= 1.0569 mol N2
Similarly,
= 1.0569 mol NH4NO3 x ( 1 mol O2 / 2 mol NH4NO3)
= 0.5285 mol O2
Similarly,
= 1.0569 mol NH4NO3 x ( 4 mol H2O / 2 mol NH4NO3)
= 2.114 mol H2O
Convert the moles of each product to grams by using the molar masses as follows:
The molar mass of N2 = 28.0134 g/mol
The molar mass of O2 = 31.9988 g/mol
The molar mass of H2O = 18.02 g/mol
Now,
= 1.0569 mol N2 x (28.0134 g N2 /1 mol N2)
= 29.6 g N2
Similarly,
= 0.5285 mol O2 x (31.9988 g O2 /1 mol O2)
= 16.9 g O2
Similarly,
= 2.114 mol H2O x (18.02 g H2O /1 mol H2O)
= 38.1 g H2O
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Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substance...