P1V1 = P2V2
He goes from V=280 mL to a total of 755 mL. Calculate P for He.
Same formula for Ar. It goes from 475 mL to 755 mL. Remember Dalton's Law which says that the partial pressure of a gas in a container is independent of any other gases present (as long as they don't react).
"A 280ml flask contains pure helium at a pressure of 754 torr . A second flask with a volume of 475ml contains pure argon at a pressure of 732 torr . If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of helium? What is the partial pressure of argon?"
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