Dust particles in the air
Chlorine is used in swimming pools to kill unwanted bacteria and keep swimmers safe from infections and disease from the water. While there isn't enough chlorine in swimming pools to cause permanent damage, it can leave your hair dry and your skin irritated and red.
Answer:
Explanation:
From the information given:
Step 1:
Determine the partial pressure of each gas at total Volume (V) = 4.0 L
So, using:





![Total pressure= P [N_2] + P[Ar] \ \\ \\ . \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ = (0.525 + 1.7)Bar \\ \\ . \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ = 2.225 \ Bar](https://tex.z-dn.net/?f=Total%20pressure%3D%20P%20%5BN_2%5D%20%2B%20P%5BAr%5D%20%5C%20%5C%5C%20%5C%5C%20.%20%5C%20%5C%20%20%5C%20%5C%20%20%5C%20%5C%20%20%5C%20%5C%20%5C%20%5C%20%20%20%5C%20%5C%20%5C%20%5C%20%5C%20%5C%20%5C%20%5C%20%3D%20%280.525%20%2B%201.7%29Bar%20%5C%5C%20%5C%5C%20.%20%5C%20%5C%20%20%5C%20%5C%20%20%5C%20%5C%20%20%5C%20%5C%20%5C%20%5C%20%20%20%5C%20%5C%20%5C%20%5C%20%5C%20%5C%20%5C%20%5C%20%3D%202.225%20%5C%20Bar)
Now, to determine the final pressure using different temperature; to also achieve this, we need to determine the initial moles of each gas.
According to Ideal gas Law.

For moles N₂:



For moles of Ar:





Finally;
The final pressure of the mixture is:

P = 2.217 atm
P ≅ 2.24 bar