Automobile air bags inflate following a serious impact.
Automobile air bags inflate following a serious impact. The impact triggers the following chemical reaction:
2 NaN3(s) → 2 Na(s)+3 N2(g)
Part A
If an automobile air bag has a volume of 11.7 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.
Homework Answers
Inflating an airbag
Automobile air bags inflate following a serious impact. The impact triggers the following chemical reaction.2NaN3(s)->2Na(s)+3N2(g)If an automobile air bag has a volume of 11.3L , what mass of NaN3 (in g ) is required to fully inflate the air bag upon impact? Assume STP conditions.
(a) Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s) What volume of...
(a) Oxygen gas reacts with powdered aluminum according to the following reaction: 4Al(s)+3O2(g)→2Al2O3(s) What volume of O2 gas, measured at 771 mmHg and 35 ∘C, is required to completely react with 54.1 g of Al? (b) Automobile air bags inflate following a serious impact. The impact triggers the following chemical reaction. 2NaN3(s)→2Na(s)+3N2(g) If an automobile air bag has a volume of 12.2 L , what mass of NaN3 (in g) is required to fully inflate the air bag upon impact?...
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags....
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags. What mass of sodium azide is needed to provide the nitrogen needed to inflate a 70.0 L bag to a pressure of 1.3 atm at 25°C? 2 NaN3 (s) → 2 Na (s) + 3 N2(g)
The air bags in cars inflate through the explosive decomposition of a solid to produce a...
The air bags in cars inflate through the explosive decomposition of a solid to produce a gas. The simplified version of the reaction that takes place in most air bags is shown. 2NaN3(s) — 2Na(s) + 3N2(8) (a) If a typical air bag has a volume of 67.0 L when inflated, how much NaNz (in grams) is required to inflate an air bag at STP? (h) Would vou want to rely on an air bag that contained only
The sodium azide required for automobile air bags is made by the reaction of sodium metal...
The sodium azide required for automobile air bags is made by the reaction of sodium metal with dinitrogen monoxide in liquid ammonia: You have 62.8 g of sodium, a 35.5-L flask containing N2O gas with a pressure of 2.48 atm at 23 °C, and excess ammonia. What is the theoretical yield (in grams) of NaN3? 3 N2O (g) + 4 Na (s) + NH3 (l) ---> NaN3 (s) + 3 NaOH (s) + 2 N2 (g) Mass = g
8. What mass of NaN3 is needed to inflate an 18.0 L air bag in an...
8. What mass of NaN3 is needed to inflate an 18.0 L air bag in an automobile at 25.0°C and 1.00 atm according to the following reaction? 6NaN3(s) + Fe2O3(s) + 3Na2O(s) + 2Fe(s) + 9N2(g)
8. What mass of NaN3 is needed to inflate an 18.0 L air bag in an automobile at 25.0°C and 1.00 atm according to th...
8. What mass of NaN3 is needed to inflate an 18.0 L air bag in an automobile at 25.0°C and 1.00 atm according to the following reaction? 6NaN3(s) + Fe2O3(s) + 3Na2O(s) + 2Fe(s) + 9N2(9)
1. Air bags are activated when a severe impact causes a steel ball to compress a...
1. Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction: 2Na (s) 3N2 (g) 2NAN3 (s) 72.01 IL1,01(3) What mass of NaN3 (s) must be reacted to inflate an air bag to 70.0 L at 1 atm and 20°C? (8 pts.) 1273,15 293.15 21100,8 0V mol HOTS 3,31 X10 2. Exactly 50.0 mL liquid...
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen...
Automobile air bags inflate during a crash or sudden stop by the
rapid generation of nitrogen gas from sodium azide, according to
the reaction:
2NaN3 (s) 2Na (s) + 3N2 (g)
How many grams of sodium azide are needed to provide sufficient
nitrogen gas to fill a 40.0 × 40.0 × 25.0 cm bag to a pressure of
1.13 atm at 23.0 °C?
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen...
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide, according to the reaction: 2NaN3(s) -----2Na(s)+3N2(g) How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 30.0 × 30.0 × 25.0 cm bag to a pressure of 1.07 atm at 12.0 °C?
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags. What mass of sodium azide is needed to provide the nitrogen needed to inflate a 70.0 L bag to a pressure of 1.3 atm at 25°C? 2 NaN3 (s) → 2 Na (s) + 3 N2(g)
The air bags in cars inflate through the explosive decomposition of a solid to produce a gas. The simplified version of the reaction that takes place in most air bags is shown. 2NaN3(s) — 2Na(s) + 3N2(8) (a) If a typical air bag has a volume of 67.0 L when inflated, how much NaNz (in grams) is required to inflate an air bag at STP? (h) Would vou want to rely on an air bag that contained only
8. What mass of NaN3 is needed to inflate an 18.0 L air bag in an automobile at 25.0°C and 1.00 atm according to the following reaction? 6NaN3(s) + Fe2O3(s) + 3Na2O(s) + 2Fe(s) + 9N2(g)
8. What mass of NaN3 is needed to inflate an 18.0 L air bag in an automobile at 25.0°C and 1.00 atm according to the following reaction? 6NaN3(s) + Fe2O3(s) + 3Na2O(s) + 2Fe(s) + 9N2(9)
1. Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction: 2Na (s) 3N2 (g) 2NAN3 (s) 72.01 IL1,01(3) What mass of NaN3 (s) must be reacted to inflate an air bag to 70.0 L at 1 atm and 20°C? (8 pts.) 1273,15 293.15 21100,8 0V mol HOTS 3,31 X10 2. Exactly 50.0 mL liquid...
Automobile air bags inflate during a crash or sudden stop by the
rapid generation of nitrogen gas from sodium azide, according to
the reaction:
2NaN3 (s) 2Na (s) + 3N2 (g)
How many grams of sodium azide are needed to provide sufficient
nitrogen gas to fill a 40.0 × 40.0 × 25.0 cm bag to a pressure of
1.13 atm at 23.0 °C?
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