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.?

We have a 275-mL flask with helium at 752 torr and a 475-mL flask with argon at 722 torr. If both flasks are connected, the partial pressure of helium will be 276 torr, the partial pressure of argon will be 457 torr and the total pressure will be 733 torr.

We have 2 flasks:

If the two flasks are connected through a stopcock and the stopcock is opened, the final volume will be the sum of the initial volumes.

Assuming ideal behavior and constant temperature, we can calculate the final partial pressure of each gas using Boyle's law.

The total pressure will be the sum of the partial pressures.

We have a 275-mL flask with helium at 752 torr and a 475-mL flask with argon at 722 torr. If both flasks are connected, the partial pressure of helium will be 276 torr, the partial pressure of argon will be 457 torr and the total pressure will be 733 torr.

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Total pressure = 732.9 torr

Partial pressure of helium =275.7 torr

Partial pressure of  argon = 457.2 torr

Explanation:

Given data:

Volume of flask one = 275 mL

Pressure of helium = 752 torr

Volume of second flask = 475 mL

Pressure of argon = 722 torr

What is partial pressure = ?

What is total pressure = ?

Solution:

V₂ = 275 mL + 475 mL = 750 mL

For helium:

P₁V₁ = P₂V₂

P₂ = P₁V₁ /V₂

P₂ =  752 torr. 275 mL /  750 mL

P₂ = 206800 torr. mL  /750 mL

P₂ = 275.7 torr

For argon:

P₁V₁ = P₂V₂

P₂ = P₁V₁ /V₂

P₂ =  722 torr. 475 mL /  750 mL

P₂ = 342950 torr. mL  /750 mL

P₂ = 457.2  torr

Total pressure = P(helium) + P ( argon)

Total pressure = 275.7 torr +  457.2  torr

Total pressure = 732.9 torr

i would say b

explanation:

but i think i would need more information than that

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