In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition...
In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition of sodium azide (NaN3) to its elements. A 58.6−g sample of sodium azide was decomposed, and the nitrogen gas generated was collected over water at 26°C. The total pressure was 733.2 mmHg. How many liters of dry N2 were generated?
Homework Answers
Answer:-
From the given data, firstly a balanced chemical equation is written then using the stoichiometry, moles of nitrogen is calculated then volume is calculated.
The answer is given in the image,
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In a collision of sufficient force, automobile air bags respond
by electrically triggering the explosive decomposition...
In a collision of sufficient force, automobile air bags respond by electrically triggering the ex...
In a collision of sufficient force, automobile air bags respond
by electrically triggering the explosive decomposition of sodium
azide (NaN3) to its elements. A 43.398 g sample of
sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7 K and 2.3...
Help? Q2) In a collision of sufficient force, automobile air bags respond by electrically trigger...
Help?
Q2) In a collision of sufficient force, automobile air bags
respond by electrically triggering the explosive decomposition of
sodium azide (NaN3) to its elements. A 43.398 g sample
of sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
Q3) An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaNz (s) + 2 Na (s) + 3 N2(g) If an air bag has a volume of 47.2 L and is to be filled with nitrogen gas at a pressure of 1.02 atm at a temperature of 24.1°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaNz (s) → 2 Na (s) + 3 N2(g) If an air bag has a volume of 43.8 L and is to be filled with nitrogen gas at a pressure of 1.13 atm at a temperature of 22.4°C, how many moles of NaN3 must decompose? You may assume the Ny behaves as an ideal gas. If Carmen adds zeros...
A sample of sodium azide (NaN 3), a compound used in automobile air bags was thermally...
A sample of sodium azide (NaN 3), a compound used in automobile air bags was thermally decomposed and 15.3 mL of nitrogen gas was collected at 25°C and 755 torr. How many grams of nitrogen were collected?
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)
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g) a....
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)→2Na(s)+3N2(g) a. How many moles of N2 are produced by the decomposition of 1.70 mol of NaN3? b. How many grams of NaN3 are required to form 13.0 g of nitrogen gas? c. How many grams of NaN3 are required to produce 11.0 ft3 of nitrogen gas if the gas has a density of 1.25 g/L?
Airbags in your car deploy through the explosive decomposition of sodium azide (NaN3) into its individual...
Airbags in your car deploy through the explosive decomposition of sodium azide (NaN3) into its individual elements (think about what this means you need to do). If 50.0g of sodium azide decomposes and fills a 68.5L airbag at a pressure of 1185.2 torr with N2 gas, what is the temperature of the gas in the airbag? (Assume N2 is a REAL gas with constants a = 1.39L2atm/mol2 and b=0.0391L/mol)
When sensors in a car detect a collision, they cause the reaction of sodium azide, NaN3,...
When sensors in a car detect a collision, they cause the reaction of sodium azide, NaN3, which generates nitrogen gas to fill the air bags within 0.03 s. 2NaN3(s)→2Na(s)+3N2(g) How many liters of N2 are produced at STP if the air bag contains 101 g of NaN3? Express your answer with the appropriate units.
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaNz. 2 NaNz (s) → 2 Na (s) + 3 N2 (g) If an air bag has a volume of 42.7 L and is to be filled with nitrogen gas at a pressure of 1.16 atm temperature of 24.9°C, how many moles of NaNg must decompose? You may assume the N2 behaves as an ideal gas. If Carmen adds zeros behind...
In a collision of sufficient force, automobile air bags respond
by electrically triggering the explosive decomposition of sodium
azide (NaN3) to its elements. A 43.398 g sample of
sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7 K and 2.3...
Help?
Q2) In a collision of sufficient force, automobile air bags
respond by electrically triggering the explosive decomposition of
sodium azide (NaN3) to its elements. A 43.398 g sample
of sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
Q3) An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7...
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaNz (s) + 2 Na (s) + 3 N2(g) If an air bag has a volume of 47.2 L and is to be filled with nitrogen gas at a pressure of 1.02 atm at a temperature of 24.1°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaNz (s) → 2 Na (s) + 3 N2(g) If an air bag has a volume of 43.8 L and is to be filled with nitrogen gas at a pressure of 1.13 atm at a temperature of 22.4°C, how many moles of NaN3 must decompose? You may assume the Ny behaves as an ideal gas. If Carmen adds zeros...
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 automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaNz. 2 NaNz (s) → 2 Na (s) + 3 N2 (g) If an air bag has a volume of 42.7 L and is to be filled with nitrogen gas at a pressure of 1.16 atm temperature of 24.9°C, how many moles of NaNg must decompose? You may assume the N2 behaves as an ideal gas. If Carmen adds zeros behind...
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