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. 2 NGN 2Na+ 3N₂ 65.009g/mol = 0.923 mol 923 mol (2)-1.384 md .923 (22) = 0.923 mal 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). K₂0(s) + S Na20(s) + N₂(g) 10 Na(s) + 2 KNO3(s) → -0.0923 mol 0.923 (1) c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually produced? 1.169 +0.078=1247 mol 1. 384 mal (845) = 1.169 md 0.093 mol (845) = 0.078 mol 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.)
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. 2 NGN 2Na+ 3N₂ 65.009g/mol = 0.923 mol 923 mol (2)-1.384 md .923 (22) = 0.923 mal 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). K₂0(s) + S Na20(s) + N₂(g) 10 Na(s) + 2 KNO3(s) → -0.0923 mol 0.923 (1) c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually produced? 1.169 +0.078=1247 mol 1. 384 mal (845) = 1.169 md 0.093 mol (845) = 0.078 mol 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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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Part d and e
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.
ZNANS
60.09
65.009g/mol =0.923 mol
-2Na+ 3N2
923 mol (3)=1.384 mdl
923 (23) = 0.923 mol
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).
_10_Na(s) + 2 KNO3(s) →
K₂0(s) + S Na₂0(s) +
N₂(g)
-0.0923 mol
0.923 (1)
c. If the overall process (both reactions) is 84.5 % efficient, how many moles of nitrogen gas are actually
produced?
1.169 +0.078 =
247 mol
1₁384 mal (84.5) = 1.169 md
0.093 mol (845) = 0.078 mol
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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