Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
Section: Chapter Questions
Problem 85E: Propane, C3H8, is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for...
See similar textbooks
icon
Related questions
icon
Concept explainers
Question
100%
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.)
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 4 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermochemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
World of Chemistry, 3rd edition
World of Chemistry, 3rd edition
Chemistry
ISBN:
9781133109655
Author:
Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:
Brooks / Cole / Cengage Learning
SEE MORE TEXTBOOKS