Problem: A 280-mL flask contains pure helium at a pressure of 753 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 723 torr .If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of helium?

FREE Expert Solution

Calculate the final pressure using Boyle's Law:

P1V1=P2V2

P1 = 753 torr

V1 = 280 mL

V2 = 280 mL + 480 mL = 760 mL

82% (202 ratings)
View Complete Written Solution
Problem Details

A 280-mL flask contains pure helium at a pressure of 753 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 723 torr .

If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of helium?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Ideal Gas Law Derivations concept. You can view video lessons to learn The Ideal Gas Law Derivations. Or if you need more The Ideal Gas Law Derivations practice, you can also practice The Ideal Gas Law Derivations practice problems.