(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a...

Question

Question

(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) 2 Na(s) +3 N2(g) An

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Answer #1

According to ideal gas law PV = nRT p is the pressure V is the volume n is number of moles R = 0.0821 L. atm. mol.kt t is the No = PV RT N = (latime) (524) (0.082)L.atm. montaxe) (25273)x MN = 2.1284 moles. Let x be the mass of NaNg required to produ

Add a comment

Answer 2

Similar Homework Help Questions

(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a...

(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a canister: 2 NaN3(s) → 2 Na(s) + 3 N2(g) An average driver's side airbag has a volume of 52L. How many grams of NaNz do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
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...

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...
Automobile airbags contain sodium azide, NaN3. It decomposes to form sodium and nitrogen gas; the nitrogen...

Automobile airbags contain sodium azide, NaN3. It decomposes to form sodium and nitrogen gas; the nitrogen inflates the airbag. How many grams of NaNg are needed to inflate an airbag to a volume of 65 Lat 2.5 atm and 25 °C?
A vehicle airbag uses a gas generator that contains a mixture of three compounds: NaN3, KNO3,...

A vehicle airbag uses a gas generator that contains a mixture of three compounds: NaN3, KNO3, and SiO2. A series of three reactions is used to convert the highly toxic sodium azide, NaN3, into N2 gas and harmless silicate glass. The nitrogen gas fills up the airbag, causing it to rapidly expand in a head-on collision. Balance the reactions involved in the deployment of an airbag by inserting the appropriate coefficients. 1. NaN3(s)--> Na(s)+N2(g) 2. Na (s)+ KNO3(s)--> K2O(s)+N2(g) 3....

O words Question 9 5 pts The air bags in automobiles were once inflated by nitrogen...

O words Question 9 5 pts 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 N, (g) If an air bag has a volume of 58.3 L and is to be filled with nitrogen gas at a pressure of 1.06 atm at a temperature of 22.1°C, how many moles of NaN3 must decompose? You may assume the Ny behaves as...
Airbags uses the decomposition of sodium azide for inflation. How many moles of sodium azide, NaN3,...

Airbags uses the decomposition of sodium azide for inflation. How many moles of sodium azide, NaN3, would have to decompose to produce 253,000,000 molecules of nitrogen gas N2? 2NaN3(s) 2Na(s) + 3N2
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid...

QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation 2 NaN3(s) - 2 Na(s) + 3 N2(9) Using stoichiometry and the ideal gas law, calculate the mass (ing) of NaN3 required to provide 42 L of N2(g) at 28.3 °C and 1.00 atm?

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)

(4) An airbag is inflated by the decomposition of sodium azide into nitrogen gas in a...

Homework Answers