9. (2 points) Though wizards might be able to manage without air-bags, Muggles certainly need them!...
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:2NaN3(s) → 2Na(s)+3N2(g)How many moles of N2 are produced by the decomposition of 3.55 mol of sodium azide?10.71.185.332.371.78
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...
Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2NaN3(s)?2Na(s)+3N2(g) How many moles of N2 are produced by the decomposition of 1.70 mol of NaN3?
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 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?
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) +3N2 (8) V 1st attempt See Periodic Table D See Hint 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 1.13 atm at 23.0 °C? g sodium azide
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?
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...
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...