Answer:-
Firstly a balanced decomposition reaction is written then using the simple concept of stoichiometry, moles of nitrogen are calculated then volume is calculated at STP.
The answer is given in the image,
Air bags in cars inflate when an elect rical spark activates sodium azide (NaN₃) so that...
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN 3 (5) — 2Na (s) + 3N 2 (9) How many grams of sodium azide are required to produce 21.0 g of nitrogen? 0 32.5 01.12 O 0.500 73.1 48.7
Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s)→2Na(s)+3N2(g) How many grams of sodium azide are required to produce 30.5 g of nitrogen?
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
A sample of sodium azide (NaN 3), a compound used in automobile air bags was thermally decomposed and 15.3 mL of nitrogen gas was collected at 25°C and 755 torr. How many grams of nitrogen were collected?
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?
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?
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)
Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed to form solid sodium and dinitrogen gas. What concerns do you think automotive air bag designers considered when selecting this reaction for their product? What would you have to consider in order to determine the appropriate amount of sodium azide to include in an automotive air bag?
10. Sodium azide decomposes rapidly to produce nitrogen gas. 2 NaN (s) 2 Na(s) + 3 N (g) How many gram of sodium azide is required to inflate a 60.0 L airbag for a car to a pressure of 1.50 atm at 32 °C? (R=0.08206 L atm/mol-K) a. 2.40 g b. 67.2 g 156 g d234 g e. 351 g
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?