00:05
In this question, we were told about automobile airbags inflate by this chemical reaction, and were asked if an airbag had a volume of 11 .8 liters, how much n .a .3 in grams, we need to fully inflate the airbag at stp.
00:24
So, stp is standard temperature and pressure.
00:26
It's 273 kelvin and one atmosphere.
00:29
So what i'm going to do is use this volume of 11 .8 liters, and my temperature and pressure here to find the number of moles of n2 gas that i would need to fully inflate it to that 11 .8 liters and then convert this moles of n2 into moles of n a or n3 and then we'll convert that to grams.
00:50
So we'll use the ideal gas law to do that that is pv equals nr t where p is pressure v is volume n is the number of moles that's what we're looking for.
01:03
R is a constant and t is temperature so the pressure is 1 atmosphere, volume is 11 .8 liters, n is what we're looking for.
01:13
R is a constant, it's 0 .0821 liter atmosphere per mole kelvin, and then t is 273 kelvin.
01:23
So if we solve for n here, we get an n of 0 .5 to 6 moles of n2, and then we'll convert that to moles of n2, and then we'll convert that to moles of n...