A275-ml flask contains pure helium at a pressure of 752 torr. a second flask with a volume of 475 ml contains pure argon at a pressure of 722 torr. if the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of each gas and the total pressure?

Explanation:

Assuming temperature remains constant, we can use Boyle's law to solve this problem: P₁V₁=P₂V₂.

Once the two flasks are connected and the stopock opened, the total volume is:

Now we use Boyle's law twice, to calculate the new pressure of each gas:

P₂He = 276 torr

P₂Ar = 457 torr

Finally we calculate the total pressure, adding the partial pressures:

it is the most commonly accepted one