This problem is providing the volume, pressure and temperature at which nitrogen gas is contained in a metallic cylinder. Thus the moles present in there are required and found to be 1.63 mol after the following calculations.
In chemistry, volume-temperature-mole-pressure behavior of gases can be studied at basic level with the ideal gas equation, relating these variables and the universal gas constant. In such a way, we can write:
[tex]PV=nRT[/tex]
Where we want to solve for n as the moles of the gas:
[tex]n=\frac{PV}{RT}[/tex]
Whereas the pressure should be in atmospheres and the temperature in kelvins as we use 0.08206 as R. Hence, we proceed as follows:
[tex]n=\frac{2000kPa*\frac{1atm}{101.325kPa}*2L}{0.08206\frac{atm*L}{mol*K}*(22+273)K}\\\\n=1.63mol[/tex]
Learn more about ideal gases: brainly.com/question/8711877
