air bags actived when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. this causes NaN3 to decompose explosively according to the following reaction:
2NaN3(s)=2Na(s)+3N2(g)
what mas of NaN3 must be reacted to inflate an air bag to 70.0L at 0C & 1.00 atm?
is this correct:
n(N2): PV/RT
n=1.00 atm x 70.0L/0.0821(L*atm/mol*K) x273K = 3.12 mol N2
mass NaN3 reacted:
(3.12 mol N2) x (2mol NaN3/3molN2)x (65.02gNaN3/1molNaN3)= 135g NaN3
please let me know if I'm doing this correct and where can I find more examples to practice more, have my test tomorrow...thankx. :)
No one has answered this question yet.
It looks good to me.
thank you for all your help Drbob222...just whish me luck for tomorrow in my test... :)
You're welcome. Good luck on your test.
Your calculations for finding the mass of NaN3 are correct. You used the ideal gas law, PV = nRT, to calculate the number of moles of N2 gas, and then used stoichiometry to convert moles of N2 to moles of NaN3, and finally used the molar mass of NaN3 to convert moles to grams.
To find more examples to practice similar problems, you can search for online resources or textbooks on stoichiometry and gas laws. Additionally, many chemistry textbooks have practice problems and examples that you can use to improve your skills. You can also ask your teacher or classmates for more practice problems or clarification on any concepts you're struggling with. Good luck on your test!