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30 January, 06:00

If the temperature is held constant during this process and the final pressure is 683 torrtorr, what is the volume of the bulb that was originally filled with gas?

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  1. 30 January, 06:11
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    Let the volume of the unknown bulb = X L

    The volume of the system, after opening valve = (X + 0.72 L)

    Use Boyles law gas equation,

    P1V1 = P2V2 (at temperature is constant)

    Given:

    P1 = 1.2 atm

    P2 = 683 torr

    Converting mmHg to atm,

    1 atm = 760 mmHg (torr)

    683 mmHg = 683/760

    = 0.8987 atm

    1.2X = 0.8987 * (X + 0.720)

    1.2X = 0.8987X + 0.6471

    0.3013X = 0.6471

    X = 2.15 L
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