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11Alexandr11 [23.1K]
3 years ago
10

A 275-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 p

ressure 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?
Chemistry
1 answer:
hichkok12 [17]3 years ago
4 0

Answer:

  • Partial pressure He = 276 torr
  • Partial pressure Ar = 457 torr
  • Total pressure = 733 torr

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:

  • 275 + 475 = 750 mL

Now we use Boyle's law <em>twice</em>, to <u>calculate the new pressure of </u><em><u>each</u></em><u> gas</u>:

  • He ⇒ 752 torr * 275 mL = P₂He * 750 mL

P₂He = 276 torr

  • Ar ⇒ 722 torr * 475 mL = P₂Ar * 750 mL

P₂Ar = 457 torr

Finally we <u>calculate the total pressure</u>, adding the partial pressures:

  • Total pressure = P₂He + P₂Ar = 733 torr
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<h3>Further explanation</h3>

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