Question

Air-bags can be inflated by the decomposition of sodium azide, NaN3. At 25.0◦C and 1.10 atm, what volume of N2(g) is produced by the decomposition of 71.4 g NaN3 under the following chemical reaction: 2NaN3(s) → 2Na(l) + 3N2(g)

Answer 1

Answer:

V = 36.7L of $N_{2}$

Explanation:

1. Write the chemical reaction for the decomposition of sodium azide:

$_{2}NaN_{3}(l)=_{2}Na(s)+_{3}N_{2}(g)$

2. Find the number of moles of $N_{2}$ produced by the decomposition of 71.4g of $NaN_{3}$:

$71.4gNaN_{3}*\frac{1molNaN_{3}}{65gNaN_{3}}*\frac{3molesN_{2}}{2molesNaN_{3}}=1.65molesN_{2}$

3. Use the ideal gas equation to find the Volume of $N_{2}$ occupied by 1.65 moles of $N_{2}$, at the temperature and pressure given by the problem:

$PV=nRT$

Solving for V:

$V=\frac{nRT}{P}$

Converting the temperature from ◦C to K:

25◦C+273.15=298.15K

Replacing values:

$V=\frac{1.65mol*(0.082\frac{atm.L}{mol.K})*298.15K}{1.10atm}$

V=36.7L of $N_{2}$