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Anni [7]
3 years ago
15

A 255-mL flask contains pure helium at a pressure of 746 torr . A second flask with a volume of 475 mL contains pure argon at a

pressure of 726 torr . If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of helium? If the two flasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of argon?
If the two flasks are connected through a stopcock and the stopcock is opened, what is the total pressure?
Chemistry
1 answer:
Pepsi [2]3 years ago
4 0

Answer:

pHe = 261 torr

pAr = 472 torr

P = 733 torr

Explanation:

The final volume for both gases is the same: V₂ = 255 mL + 475 mL = 730 mL

We can find the final partial pressure of each gas using Boyle's law.

He

P₁ × V₁ = P₂ × V₂

P₂ = P₁ × V₁ / V₂

P₂ = 746 torr × 255 mL / 730 mL = 261 torr

Ar

P₁ × V₁ = P₂ × V₂

P₂ = P₁ × V₁ / V₂

P₂ = 726 torr × 475 mL / 730 mL = 472 torr

The total pressure is the sum of the partial pressures.

P = 261 torr + 472 torr = 733 torr

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C

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2.11 x 10²⁴ molecules.

Explanation:

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The correct order it b. always add acid last.

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Answer:

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