Grade 11 Nitrogen gas makes up almost 80% of our atmosphere.

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Grade 11
Nitrogen gas makes up almost 80% of our atmosphere.What is the density of pure nitrogen gas,in g/L,at 12.50 degree and 126.63 kPa?

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Use the Gas Law:PV=nRT.Therefore,n=PV/(RT)=1.25atm( you gotta convert kPa to atm) *V (you don't have to calculate this cuz you'll never know) / ( .0821 L atm mol^-1 K^-1 * 285.65K) =.053301*V mol N2 gas
calculate the mass of that much of N2 gas:.053301*V mol * ( 2* 14.01g/mol)=1.493*V(remember V is a constant here) g N2
Density=mass/volume=1.493*V/V=1.493 g/L
Always remember that you don't have to figure out every single variable in the question,using substitution is the best way.

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