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(g) Calculate the mass of each product gas if 1.29 g of ammonium nitrate reacts. N2 g O2 g H2O g
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(g) Calculate the mass of each product gas if 1.29 g of ammonium nitrate reacts. N2 g O2 g H2O g
Introductory Chemistry: A Foundation
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ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 10QAP
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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(g)
Calculate the mass of each product gas if 1.29 g of ammonium nitrate reacts.
N2 | g |
O2 | g |
H2O | g |
Expert Solution
Given
NH4NO3(s) → N2(g) + O2(g) + H2O(g)
Mass of ammonium nitrate = 1.29 g
To calculate the mass of product in the reaction , first convert this mass of reactant to moles .
From this moles of reactant , Calculate the moles of product formed.
At the end convert this Moles to mass , to get final answer
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