3 attempts let Check my work Enter your answer in the provided box. The air bags

Question

3 attempts let Check my work Enter your answer in the provided box. The air bags in cars are inflated when a collision triggers the explosive, highly exothermic decomposition of sodium azide (NaN3): 2NaN3(s) 2Na(s) + 3N2(g) The passenger-side air bag in a typical car must fill a space approximately four times as large as the driver-side bag to be effective. Calculate the mass of sodium azide required to fill a 136-L air bag. Assume the pressure in the car is 1.00 atm and the temperature of N2 produced is 85°C. References eBook & Resources Multipart

Explanation / Answer

1st calculate the mol of N2 required:
Given:
P = 1.0 atm
V = 136.0 L
T = 85.0 oC
= (85.0+273) K
= 358 K

find number of moles using:
P * V = n*R*T
1 atm * 136 L = n * 0.08206 atm.L/mol.K * 358 K
n = 4.629 mol

from reaction,
mol of NaN3 used = (2/3)*moles of N2 required
= (2/3)*4.629 mol
= 3.086 mol

Molar mass of NaN3,
MM = 1*MM(Na) + 3*MM(N)
= 1*22.99 + 3*14.01
= 65.02 g/mol

use:
mass of NaN3,
m = number of mol * molar mass
= 3.086 mol * 65.02 g/mol
= 200 g
Answer: 200 g

Related Questions

Navigate

• Browse (All)
• Browse 3
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.