Question

A sample of nitrogen (N2) gas in a 10.0L container has a

pressure of 1.0 atm at 297 K. Assuming ideal gas behavior,
what will the pressure be if the same amount of nitrogen
gas is put into a 5.0L container at 297 K?

Answer 1

Answer: The pressure of nitrogen will be 2.0 atm

Step-by-step explanation:

According to ideal gas equation:

`PV=nRT`

P = pressure of gas = 1.0 atm

V = Volume of gas = 10.0 L

n = number of moles = ?

R = gas constant =
`0.0821Latm/Kmol`

T =temperature =
`297K`

`n=(PV)/(RT)`

`n=(1.0atm* 10.0L)/(0.0820 L atm/K mol* 297K)=0.41moles`

Now again using ideal gas equation :

`P=(nRT)/(V)=(0.41mol* 0.0821Latm/Kmol* 297K)/(5.0L)=2.0atm`

Thus pressure of nitrogen will be 2.0 atm