Achieve weeks3-4 question 14

[605815546]

Hi, I've been really stuck on this problem and i'm not sure what i'm doing wrong. I found the volume of N2 and i tried plugging it into the w= -P(delta V) equation but keep getting it wrong. Does pressure stay the same at 1.00 atm? if not, how do we calculate the new pressure?

"Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag.

2NaN3(s)⟶2Na(s)+3N2(g)

Calculate the value of work, w, for the system if 11.9 g NaN3 reacts completely at 1.00 atm and 22ºC."

[George]

For this problem you will use the equation w = -delta n * R (8.3145) * T (in Kelvins which is 295.15K for this problem).
In order to do this problem you have to find the delta n of moles and plug it into the equation. In order to do that you will transfer 11.9g NaN3 into mols by dividing by 64.99g and then you will multiple by 1.5 in order to turn moles NaN3 into moles N2. And since the moles N2 is the only gas (thus is the only thing that can be used in this equation) the delta n is equal to the moles of N2

[Dayeon Kim 2D]

The pressure does stay the same but once you found work then you need to change it to joules by multiplying it by 101.325J because the units are still in L*atm.