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7 June, 08:30

A 275-mL f lask contains pure helium at a pressure of 752 torr. A second f lask with a volume of 475 mL contains pure argon at a pressure of 722 torr. If the two f lasks are connected through a stopcock and the stopcock is opened, what is the partial pressure of each gas and the total pressure?

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  1. 7 June, 08:46
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    The partial pressure of Helium is 275.7 torr

    The partial pressure of argon is 457.3 torr

    The total pressure is 733 torr

    Explanation:

    Step 1: Data given

    Volume helium flask = 275 mL = 0.275L

    Pressure in helium flask = 752 torr

    Volume argon flask = 475 mL = 0.475 L

    Pressure in argon flask = 722 torr

    Step 2: Calculate the total volume of the gas mixture once the stopcock is opened.

    Total volume = volume of Helium flask + volume argon flask

    Total volume = 275 + 475 = 750 mL = 0.750 L

    Step 3: Calculate partial pressure of Helium

    pHe * VHe = p'He * Vtotal

    ⇒ with pHe = the pressure of Helium = 752 torr

    ⇒ with VHe = the volume in the helium flask = 275 mL

    ⇒ with p'He = the partial pressure of helium = To be determined

    ⇒with Vtotal = the total volume = 750 mL

    p'He = (pHe*VHe) / Vtotal

    p'He = (752*275) / 750

    p'He = 275.7 torr

    Step 4: Calculate partial pressure of Argon

    pAr * VAr = p'Ar * Vtotal

    ⇒ with pAr = the pressure of Argon = 722 torr

    ⇒ with VAr = the volume in the Argon flask = 475 mL

    ⇒ with p'Ar = the partial pressure of argon = To be determined

    ⇒with Vtotal = the total volume = 750 mL

    p'Ar = (pAr * VAr) / Vtotal

    p'Ar = (722*475) / 750

    p'Ar = 457.3 torr

    Step 5: Calculate the total pressure

    Total pressure = partial pressure Helium + partial pressure Argon

    Total pressure = 275.7 torr + 457.3 torr = 733 torr
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