Airbags rapidly produce nitrogen gas through reactions like this one: 2 NaN₃ (s) $\rightarrow$ Na (s) + 3 N₂(g)
In this reaction,what volume of nitrogen gas can be produced by the reaction of 13.0 g of NaN₃ if the temperature is 350 K and the pressure is 1.2 atmospheres? The formula mass of NaN₃ = 65 g/mol.

Question

Airbags rapidly produce nitrogen gas through reactions like this one: 2 NaN₃ (s)

\rightarrow

Na (s) + 3 N₂(g)
In this reaction,what volume of nitrogen gas can be produced by the reaction of 13.0 g of NaN₃ if the temperature is 350 K and the pressure is 1.2 atmospheres? The formula mass of NaN₃ = 65 g/mol.

Quizplus · Accepted Answer

First, calculate the moles of NaN₃ reacted: $13.0 \, \text{g} \div 65 \, \text{g/mol} = 0.2 \, \text{mol}$. According to the balanced equation, 2 moles of NaN₃ produce 3 moles of N2, so 0.2 moles of NaN₃ will produce $0.3 \, \text{mol}$ of N2. Using the ideal gas law $PV = nRT$, where $P = 1.2 \, \text{atm}$, $n = 0.3 \, \text{mol}$, $R = 0.0821 \, \text{L·atm/mol·K}$, and $T = 350 \, \text{K}$, solve for $V$: $V = \frac{nRT}{P} = \frac{0.3 \times 0.0821 \times 350}{1.2} \approx 7.2 \, \text{L}$.

Airbags Rapidly Produce Nitrogen Gas Through Reactions Like This One →\rightarrow→

Airbags Rapidly Produce Nitrogen Gas Through Reactions Like This One $\rightarrow$