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 gb.124 gc.77.9 gd.107 g

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 68QRT: Cisplatin, Pt(NH3)2Cl2, a drug used in the treatment of cancer, can be made by the reaction of...

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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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