Airbags used in automobiles are inflated with nitrogen gas (28.01 g/mol) produced from the reaction of sodium azide (NaN3, 65,01 g/mol) and excess iron(III) oxide (Fe2O3, 159.69 g/mol) as shown in the following equation: 6NaN3(s) + Fe2O3(s) ➜ 3Na2O(s) + 2Fe(s) + 9N2(g) An airbag contains 40.0 L of nitrogen gas at 1.10 atm and 25.0 ºC. How many grams of sodium azide is needed to completely produce all of the nitrogen in the presence of excess iron(III) oxide? Select one: a.94.8 g b.124 g c.77.9 g d.107 g
Airbags used in automobiles are inflated with nitrogen gas (28.01 g/mol) produced from the reaction of sodium azide (NaN3, 65,01 g/mol) and excess iron(III) oxide (Fe2O3, 159.69 g/mol) as shown in the following equation: 6NaN3(s) + Fe2O3(s) ➜ 3Na2O(s) + 2Fe(s) + 9N2(g) An airbag contains 40.0 L of nitrogen gas at 1.10 atm and 25.0 ºC. How many grams of sodium azide is needed to completely produce all of the nitrogen in the presence of excess iron(III) oxide? Select one: a.94.8 g b.124 g c.77.9 g d.107 g
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.87PAE
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Airbags used in automobiles are inflated with nitrogen gas (28.01 g/mol) produced from the reaction of sodium azide (NaN3, 65,01 g/mol) and excess iron(III) oxide (Fe2O3, 159.69 g/mol) as shown in the following equation:
6NaN3(s) + Fe2O3(s) ➜ 3Na2O(s) + 2Fe(s) + 9N2(g)
An airbag contains 40.0 L of nitrogen gas at 1.10 atm and 25.0 ºC. How many grams of sodium azide is needed to completely produce all of the nitrogen in the presence of excess iron(III) oxide?
Select one:
a.94.8 g
b.124 g
c.77.9 g
d.107 g
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