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6. How do airbags work? a. The rapid decomposition of sodium azide, NaN3 (MW = 65.0099 g/mol), to its elements is the first of several reactions used to inflate airbags. How many moles of gas are produced from 60.0 g of NaN3? Note: You will need a balanced chemical equation. b. As you know solid sodium is highly reactive (and we probably don't want it on our face in a car accident), the following reaction removes the solid sodium. How many moles of N₂ are produced in this reaction? Hint: You will need the number of moles of Na formed in the first reaction (part a). Na(s) + KNO3(s)→ K₂O(s) + Na₂0(s) + N₂(g) c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually produced?

6. How do airbags work? a. The rapid decomposition of sodium azide, NaN3 (MW = 65.0099 g/mol), to its elements is the first of several reactions used to inflate airbags. How many moles of gas are produced from 60.0 g of NaN3? Note: You will need a balanced chemical equation. b. As you know solid sodium is highly reactive (and we probably don't want it on our face in a car accident), the following reaction removes the solid sodium. How many moles of N₂ are produced in this reaction? Hint: You will need the number of moles of Na formed in the first reaction (part a). Na(s) + KNO3(s)→ K₂O(s) + Na₂0(s) + N₂(g) c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually produced?

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
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Problem 85E: Propane, C3H8, is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for...
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6. How do airbags work? a. The rapid decomposition of sodium azide, NaN3 (MW = 65.0099 g/mol), to its elements is the first of several reactions used to inflate airbags. How many moles of gas are produced from 60.0 g of NaN3? Note: You will need a balanced chemical equation. b. As you know solid sodium is highly reactive (and we probably don't want it on our face in a car accident), the following reaction removes the solid sodium. How many moles of N₂ are produced in this reaction? Hint: You will need the number of moles of Na formed in the first reaction (part a). Na(s) + KNO3(s) → K₂O(s) + Na₂O(s) + N₂(g) c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually produced? d. What pressure must a 60.0 L air bag be at for the actual amount of nitrogen gas produced (answer in 6c) to inflate it at 25°C? e. What would the volume of the airbag be if an accident were to occur at a much lower temperature (the average winter temperature in Deadhorse, Alaska is - 30°C)? (Assume pressure and reaction efficiency remain constant.)
Transcribed Image Text:6. How do airbags work? a. The rapid decomposition of sodium azide, NaN3 (MW = 65.0099 g/mol), to its elements is the first of several reactions used to inflate airbags. How many moles of gas are produced from 60.0 g of NaN3? Note: You will need a balanced chemical equation. b. As you know solid sodium is highly reactive (and we probably don't want it on our face in a car accident), the following reaction removes the solid sodium. How many moles of N₂ are produced in this reaction? Hint: You will need the number of moles of Na formed in the first reaction (part a). Na(s) + KNO3(s) → K₂O(s) + Na₂O(s) + N₂(g) c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually produced? d. What pressure must a 60.0 L air bag be at for the actual amount of nitrogen gas produced (answer in 6c) to inflate it at 25°C? e. What would the volume of the airbag be if an accident were to occur at a much lower temperature (the average winter temperature in Deadhorse, Alaska is - 30°C)? (Assume pressure and reaction efficiency remain constant.)
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