A certain mass of nitrogen gas occupies a volume of 2.21 L at a pressure of 1.05 atm. At what pressure will the volume of this sample be 4.59 L? Assume constant temperature and ideal behavior.

Answer 1

Hello (again), Andrea,

This problem is solved ising the same approach I outlined in a similar question in which we used the formula:

P1V1/T1 = P2V2/T2

That formula is explained in the earlier question.

I believe if you rearrange the equation to find P2, the requested pressure, and make a table for all the data (labelled P1, V1, T1, etc., that it will be easy to answet this. Since neither the moles nor the pressure change, it becomes straightforwad.

Reaarnge the equation for P2:

P2 = P1(V1/V2)(T2/T1)

Since T2 = T1,

P2 = P1(V1/V2)(T2/T1)

P2 = (1.05atm)(2.21 L/4.59 L) = 0.51 atm

Wow, fast and easy. Not even a temperature conversion to K, since there is no temperature change.

Bob