Question

The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. If an air bag has a volume of 43.8 L and is to be filled with nitrogen gas at a pressure of 1.13 atm at a temperature of 22.4˚C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas. If Carmen adds zeros behind the decimal place in your answer, do not worry. It will be graded correctly.

Answer 1

Explanation:

The given data is as follows.

        P = 1.13 atm,       V = 43.8 L

       T = $22.4^{o}C$ = (22.4 + 273) K = 295.4 K

Now, using the ideal gas equation we will find the number of moles as follows.

                   PV = nRT

 $1.13 atm \times 43.8 L = n \times 0.08206 atm L/mol K \times 295.4 K$

                      n = $\frac{49.494}{24.24}$

                     n = 2.042 mol

Thus, we can conclude that 2.042 mol  of $NaN_{3}$ must decompose.