Answer:
The pressure of the nitrogen in the container is 168.774 kPa
Explanation:
The volume, pressure, temperature and mol of a gas are linked through the ideal gas law which is:
p . V = n . R . T
Where p is the pressure of the gas, V the volume of the gas, n the amount of moles of the gas, T the temperature of the gas and R the universal gas constant.
The universal gas constant R we will be using is:
[tex]R= 8.314\frac{L . kPa}{K . mol}[/tex]
For example, What is the temperature of 4 mol of gas in a 10 Liters container at 300kPa?
The data is:
V = 10L
p = 300kPa
n = 4 moles
[tex]R= 8.314\frac{L . kPa}{K . mol}[/tex]
T = ?
Now we put the data in the equation and calculate the temperature.
10L ⋅ 300kPa = 4mol ⋅ [tex] 8.314\frac{L . kPa}{K . mol}[/tex] ⋅ T
T = 10L· 300kPa÷4mol ⋅ [tex]8.314\frac{L . kPa}{K . mol}[/tex]
T= 90.21 K
So, knowing all the data except one, using the ideal gas law we can calculate it.
The equation for this case would be:
p = 0.5mol · [tex]8.314\frac{L . kPa}{K . mol}[/tex] · 203K ÷ 5.0L
And the result:
p = 168.774 kPa
