ne air bags in automobilles were once Inflated by hitrogen gas generated by the rapid decomposition oT odium azide, NaNz. 2 NaN3 (s) → 2 Na (s) + 3 N2 (g) an air bag has a volume of 58.3 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a emperature of 23.8°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an deal gas. lote: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, nter your response to four decimal places. Carmen may add or remove digits from your response, your ubmission will still be graded correctly if this happens.
ne air bags in automobilles were once Inflated by hitrogen gas generated by the rapid decomposition oT odium azide, NaNz. 2 NaN3 (s) → 2 Na (s) + 3 N2 (g) an air bag has a volume of 58.3 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a emperature of 23.8°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an deal gas. lote: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, nter your response to four decimal places. Carmen may add or remove digits from your response, your ubmission will still be graded correctly if this happens.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN₃.
Chemical Reaction:
\[ 2 \, \text{NaN}_3 \, (\text{s}) \rightarrow 2 \, \text{Na} \, (\text{s}) + 3 \, \text{N}_2 \, (\text{g}) \]
Problem Statement:
If an air bag has a volume of 58.3 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a temperature of 23.8°C, how many moles of NaN₃ must decompose? You may assume the N₂ behaves as an ideal gas.
Note: Do not use scientific notation or units in your response. Significant figures will not be graded in this question; enter your response to four decimal places. Carmen may add or remove digits from your response; your submission will still be graded correctly if this happens.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fde215326-a426-4bd9-8673-34e96dbfc9c9%2F058c5425-7fa4-48c5-a304-b80bfdea1f8d%2Fh6med6_processed.png&w=3840&q=75)
Transcribed Image Text:The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN₃.
Chemical Reaction:
\[ 2 \, \text{NaN}_3 \, (\text{s}) \rightarrow 2 \, \text{Na} \, (\text{s}) + 3 \, \text{N}_2 \, (\text{g}) \]
Problem Statement:
If an air bag has a volume of 58.3 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a temperature of 23.8°C, how many moles of NaN₃ must decompose? You may assume the N₂ behaves as an ideal gas.
Note: Do not use scientific notation or units in your response. Significant figures will not be graded in this question; enter your response to four decimal places. Carmen may add or remove digits from your response; your submission will still be graded correctly if this happens.
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