Sodium azide, \mathrm{NaN}_3, decomposes as shown.2 \mathrm{NaN... | Filo
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Sodium azide, \mathrm{NaN}_3, decomposes as shown.2 \mathrm{NaN... | Filo
Solution For Sodium azide, NaN3 , decomposes as shown.2NaN3 →2Na 3 N2 Which volume of nitrogen, measured at room temperature and pressure, will be pro
Mar 24, 2023
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SOLVED: The airbags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide; NaN3:NaN3 (s) → 2 Na (s) 3 N2 (g)If an airbag has a volume of 51.9 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a temperature of 21.4°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
SOLVED: The airbags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide; NaN3:NaN3 (s) → 2 Na (s) 3 N2 (g)If an airbag has a volume of 51.9 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a temperature of 21.4°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
numerade.com
Oct 2, 2021
Sodium azide, the explosive compound in automobile air bags, decomposes according to the following equation: 2 NaN3(s) ⟶2 Na(s) 3 N2(g) What mass of sodium azide is required to provide the nitrogen needed to inflate a 75.0-L. bag to a pressure of 1.3 atm at 25^∘ C ? | Numerade
Sodium azide, the explosive compound in automobile air bags, decomposes according to the following equation: 2 NaN3(s) ⟶2 Na(s) 3 N2(g) What mass of sodium azide is required to provide the nitrogen needed to inflate a 75.0-L. bag to a pressure of 1.3 atm at 25^∘ C ? | Numerade
numerade.com
May 12, 2020
One of the reactions used to inflate automobile air bags involves sodium azide (NaN3) : 2 NaN3(s) →2 Na(s) 3 N2(g) mass of N2 produced from the decomposition of NaN 3 shown at right. | Numerade
One of the reactions used to inflate automobile air bags involves sodium azide (NaN3) : 2 NaN3(s) →2 Na(s) 3 N2(g) mass of N2 produced from the decomposition of NaN 3 shown at right. | Numerade
numerade.com
Sep 9, 2020
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SOLVED: The airbags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide; NaN3:NaN3 (s) → 2 Na (s) 3 N2 (g)If an airbag has a volume of 51.9 L and is to be filled with nitrogen gas at a pressure of 1.03 atm and a temperature of 21.4°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas.
SOLVED: The airbags in automobiles were once inflated b…
Oct 2, 2021
numerade.com
Sodium azide, the explosive compound in automobile air bags, decomposes according to the following equation: 2 NaN3(s) ⟶2 Na(s) 3 N2(g) What mass of sodium azide is required to provide the nitrogen needed to inflate a 75.0-L. bag to a pressure of 1.3 atm at 25^∘ C ? | Numerade
Sodium azide, the explosive compound in automobile air bags…
May 12, 2020
numerade.com
One of the reactions used to inflate automobile air bags involves sodium azide (NaN3) : 2 NaN3(s) →2 Na(s) 3 N2(g) mass of N2 produced from the decomposition of NaN 3 shown at right. | Numerade
One of the reactions used to inflate automobile air bags involves sodi…
Sep 9, 2020
numerade.com
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Sodium azide (NaN3, molar mass = 65.01 g/mol) rapidly decompose... …
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Sodium azide (NaN3) is used in some automobile airbags. By the impact of the collision, the decomposition reaction of NaN3 is as follows:2NaN3 (s) → 2Na (s) 3N2 (g)Nitrogen gas created during the collision suddenly inflates the cushion between the driver and the control panel. The volume of N2 (in liters) formed by the decomposition of 130.02 g of NaN3 at 80 ℃ and 823 mmHg can be calculated. (NaN3: 65.01 g/mol)
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