AP EAMCET · Chemistry · States of Matter
A car airbag is inflated by \(\mathrm{N}_2\) produced during rapid decomposition of \(\mathrm{NaN}_3(s)\). What will be the pressure of the inflated airbag if \(130 \mathrm{~g}\) of \(\mathrm{NaN}_3\) is used. The volume of airbag is \(10 \mathrm{~L}\left(T=300 \mathrm{~K}, R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)\)
- A \(7.38 \mathrm{~atm}\)
- B \(4.92 \mathrm{~atm}\)
- C \(3.0 \mathrm{~atm}\)
- D \(9.84 \mathrm{~atm}\)
Answer & Solution
Correct Answer
(A) \(7.38 \mathrm{~atm}\)
Step-by-step Solution
Detailed explanation
Given that, \(2 \mathrm{NaN}_3 \rightleftharpoons 2 \mathrm{Na}+3 \mathrm{~N}_2\) Number of moles of sodium azide \(=\frac{130}{65}=2\) Number of moles of nitrogen \(=2 \times \frac{3}{2}=3\) We know that, \(V=\frac{n R T}{p}\)…
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