Question

An airbag is inflated by \(N_2\) produced during rapid decomposition of \(NaN_3(s)\). What will be the pressure of the inflated airbag if 130 g of \(NaN_3\) is used? The volume of airbag is 10 L \((T=300\ K,\ R=0.082\ L\ atm\ K^{-1}\ mol^{-1})\)

• A. 7.38 atm
• B. 4.92 atm
• C. 3.0 atm
• D. 9.84 atm

Hint:

For airbag problems, first calculate moles of gas produced from the balanced chemical equation and then apply \[ PV=nRT. \]

Answer 1

The Correct Option is A

Step 1: Balance decomposition and compute moles.
2NaN₃ → 2Na + 3N₂. n(NaN₃) = 130/65 = 2 mol → n(N₂) = 3 mol.

Step 2: Use ideal gas law for pressure.
P = nRT/V = 3×0.082×300/10 = 7.38 atm.

Step 3: Final Answer:
7.38 atm (option 1).