Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH4NO3 (s) --> N2 (g) + O2 (g) + H20 (g) Calculate the mass of each product gas if 20.0 g of ammonium nitrate reacts.
The molecular weight of ammonium nitrated is 80 g/mole.
The balance chemical equation of ammonium nitrate :
2NH4NO3 ---> 2N2 + O2 +4H2O
So 160 grams of ammonium nitrate produces 56 g Nitrogen, 32 gram Oxygen and 72 g of water.
so if 20 grams of ammonium nitrate ie 1/8 of 160 g of reactant ammonium nitrate taken than the product form will also be 1/8 .
160 x 1/8 = 20 gram ammonium nitrate taken.
Nitrogen produced 56 x 1/8 = 7 g
Oxygen produced 32 x 1/8 = 4 g
Water produced 72 x 1/8 = 9 g.
Mass of product N2 7 g, O2 4g and H2O 9 g will be produce by 20 g NH4NO3.
Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into...
Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH4NO3(s) + N2(g) + O2(g) + H2O(9) Calculate the mass of each product gas if 84.6 g of ammonium nitrate reacts. g N₂ 802 gH,0
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Q2) In a collision of sufficient force, automobile air bags
respond by electrically triggering the explosive decomposition of
sodium azide (NaN3) to its elements. A 43.398 g sample
of sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
Q3) An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7...
In a collision of sufficient force, automobile air bags respond
by electrically triggering the explosive decomposition of sodium
azide (NaN3) to its elements. A 43.398 g sample of
sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7 K and 2.3...
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