Question 12 Sodium aride is used in air bags for automobiles. The pas produced from the decomposition of sodinamide...
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.
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...
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...
Automobile air bags inflate during a crash or sudden stop by the rapid generation of nitrogen gas from sodium azide, according to the reaction: 2NaN(s) —→ 2Na(s) + 3N, (g) v 4th attempt i See Periodic Table D See How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill a 40.0 x 40.0 25.0 cm bag to a pressure of 1.21 atm at 23.0°C? 79.34 g sodium azide
1. Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed: 2NaN3 (s) ―—› 2Na(s) + 3N2(g) What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?
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?
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...
Reattempt last question below, or select another question Sodium azide, NaNg, is used in air bags because it quickly produces nitrogen gas upon decomposition, What volume, in L, of nitrogen gas should theoretically be produced from the decomposition of 10.5 grams of sodium azide on a hot Phoenix day (112°C) with a barometric pressure of 726 Torr? 2 NaNy(s) 2 Na(s) +3 N2(g) LN2 ( Enter an integer or decimal number [more..] License
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...