Question
Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction:$$2 \mathrm{NaN}_{3}(s) \longrightarrow 2 \mathrm{Na}(s)+3 \mathrm{N}_{2}(g)$$If an automobile air bag has a volume of $11.8 \mathrm{L},$ what mass of $\mathrm{NaN}_{3}(\mathrm{ing})$ is required to fully inflate the air bag upon impact? Assume STP conditions.
Step 1
We know that at STP, 1 mole of any gas occupies 22.4 L. So, we can use this to convert the volume of nitrogen gas into moles: $$\frac{11.8 \, \text{L} \, \text{N}_2}{22.4 \, \text{L/mol}} = 0.527 \, \text{mol} \, \text{N}_2$$ Show more…
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Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction: $$ 2 \mathrm{NaN}_{3}(s) \rightarrow 2 \mathrm{Na}(s)+3 \mathrm{~N}_{2}(g) $$ If an automobile air bag has a volume of $11.8 \mathrm{~L}$, what mass of $\mathrm{NaN}_{3}$ (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.
Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction: $$ 2 \mathrm{NaN}_{3}(s) \longrightarrow 2 \mathrm{Na}(s)+3 \mathrm{~N}_{2}(g) $$ If an automobile airbag has a volume of $11.8 \mathrm{~L},$ what mass of $\operatorname{NaN}_{3}($ in $g)$ is required to fully inflate the airbag upon impact? Assume STP conditions.
Automobile air bag inflate following a serious impact. The impact triggers the chemical reaction: $$ 2 \mathrm{NaN}_{3}(s) \longrightarrow 2 \mathrm{Na}(s)+3 \mathrm{N}_{2}(g) $$ If an automobile air bag has a volume of $11.8 \mathrm{L}$, how much $\mathrm{NaN}_{3}$ in grams is required to fully inflate the air bag upon impact? Assume STP conditions.
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