Homework Help: chemm

Posted by Sienna on Tuesday, April 27, 2010 at 10:44pm.

A car air bag requires 70. L of nitrogen gas to inflate properly. The following equation represents the production of nitrogen gas:

2NAN subscript 3 yielding 2NA + 3N subscript 2

the density of nitrogen gas is typically 1.16 g/L at room temperature. How would you calculate the number of grams of Nitrogen that is needed to inflate the air bag?

chemm - DrBob222, Tuesday, April 27, 2010 at 10:53pm
First let me point out that NAN3 is NOT the same as NaN3 and NA is not the same as Na.
2NaN3 ==> 2Na + 3N2

How about 1.16 g/L x 70 L = ?? g.

Answer this Question

Related Questions

Chemistry - A car air bag requires 70. L of nitrogen gas to inflate properly. ...
physics - suppose you want to design an air bag system that can protect the ...
chemistry - Air bags are actived when a servere impact causes a steel ball to ...
chem - Air bags are actived when a servere impact causes a steel ball to ...
chem - Air bags are actived when a servere impact causes a steel ball to ...
Chemistry - utomotive air bags inflate when sodium azide, NaN3, rapidly ...
chemistry - One essential step in the manufacture of many plant fertilizers is ...
chemistry - sodium azide, decomposes according to the following equation: 2NaN3...
Physics - Nitrogen gas is introduced into a large deflated plastic bag. No gas ...
Chemistry - Apply the gas laws to determine how many grams of sodium azide (NaN3...

For Further Reading

First Name:
School Subject:
Answer: