From ideal gas equation, PV = nRT
Number moles of N2(g), n= PV/RT = 1.50*60/(0.08206*305) = 3.60 moles
From the given balanced equation,
3 moles of N2 gas obtained by 2 moles of solid NaN3
3.60 moles of N2 gas obtained by 2*3.60/3 = 2.4 moles of solid NaN3
Mass of sodium azide required = 2.4*65 = 156 grams
Ans: c
10. Sodium azide decomposes rapidly to produce nitrogen gas. 2 NaN (s) 2 Na(s) + 3 N (g) How many gram of sodium az...
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?
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?
Automobile airbags contain solid sodium azide, NaN, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2 NaN,(s) — 2 Na(s) + 3N, (g) Calculate the value of work, w, for the system if 36.6 g NaN, reacts completely at 1.00 atm and 22 'C.
Automobile airbags contain solid sodium azide, NaN,, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2 NaN,(s) +2 Na(s) + 3N,(6) Calculate the value of work, w, for the system if 34.8 g Nan, reacts completely at 1.00 atm and 22 °C.
3. Air bags deployed in car accidents use a series of reactions to rapidly generate nitrogen gas in order to inflate the airbag. The first reaction is the decomposition of sodium azide (NaN,) to form nitrogen gas and solid sodium metal. The sodium metal then reacts with solid potassium nitrate to form more nitrogen gas, as well as sodium oxide and potassium oxide (both as a solid). A. Write and balance the reactions described above (including correct state for each...
Automobile airbags contain solid sodium azide, NaN,, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2 NaN,(s) + 2Na(s) + 3N, (8) Calculate the value of work, w, for the system if 17.2 g NaN, reacts completely at 1.00 atm and 22 °C.
(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 NaN3 do you need to decompose to fill the airbag with N2 at room temperature (25°C) and atmospheric pressure (1.00 atm)?
(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)?
In the reaction, 2 NaN (s) —2 Na(s) + 3 N, (g) how many liters of nitrogen, Ny measured at STP, would be produced from the decomposition of 361 g of sodium azide, NaN? Nproduced:
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)