Explanation:
Given data is as follows.
= 4 L, = 875 kPa
= (27 + 273) K = 300 K, = 13 L
= 54.9 kPa,
Total volume will be 4 L + 13 L = 17 L
Hence, calculate the total pressure as follows.
(as T is same so it will cancel out)
= 205.8 kPa
Now, using ideal gas equation we will calculate the moles of nitrogen as follows.
PV = nRT
3500 =
n = 1.4 mol
Moles of argon will be calculated as follows.
PV = nRT
713.7 =
n = 0.28 mol
Therefore, mole fraction of nitrogen will be as follows.
Mole fraction of
=
=
= 0.833
Relation between partial pressure and total pressure is as follows.
where, = partial pressure of a gas
= mole fraction of the gas
Thus, we will calculate the partial pressure of nitrogen after mixing as follows.
205.8 kPa =
Thus, we can conclude that the partial pressure of nitrogen after mixing is 247.05 kPa.