we have:
P = 1.3 atm
V = 70.0 L
T = 25.0 oC
= (25.0+273) K
= 298 K
find number of moles using:
P * V = n*R*T
1.3 atm * 70 L = n * 0.08206 atm.L/mol.K * 298 K
n = 3.719 mol
This is number of moles of N2 required
Now from reaction,
mol of NaN3 required = (2/3)*moles of N2
=(2/3)*3.719 mol
= 2.479 mol
Molar mass of NaN3 = 1*MM(Na) + 3*MM(N)
= 1*22.99 + 3*14.01
= 65.02 g/mol
we have below equation to be used:
mass of NaN3,
m = number of mol * molar mass
= 2.479 mol * 65.02 g/mol
= 161 g
Answer: 161 g
Feel free to comment below if you have any doubts or if this answer do not work
10. (10 points) Sodium azide, NaNs, is used to provide gas to inflate automobile air bags....
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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?
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Automobile air bags inflate following a serious impact. The impact triggers the following chemical reaction:2 NaN3(s) → 2 Na(s)+3 N2(g)Part AIf an automobile air bag has a volume of 11.7 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.
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?
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.
QUESTION 3 Automobile airbags use the decomposition of sodium azide, NaN3, to provide gas for rapid inflation 2 NaN3(s) - 2 Na(s) + 3 N2(9) Using stoichiometry and the ideal gas law, calculate the mass (ing) of NaN3 required to provide 42 L of N2(g) at 28.3 °C and 1.00 atm?
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?