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26 July, 03:37

A 0.100 mile sample of gas is at a temperature of 85.0 degrees C and a volume of 3.47 L. What is the pressure of the gas (in mm hg?)

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  1. 26 July, 04:04
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    Answer: 64.6 mmHg

    Explanation:

    Given that:

    Volume of gas V = 3.47L

    (since 1 liter = 1dm3

    3.47L = 3.47dm3)

    Temperature T = 85.0°C

    Convert Celsius to Kelvin

    (85.0°C + 273 = 358K)

    Pressure P = ?

    Number of moles of gas N = 0.100 mole

    Note that Molar gas constant R is a constant with a value of 0.0082 ATM dm3 K-1 mol-1

    Then, apply ideal gas equation

    pV = nRT

    p x 3.47dm3 = 0.10 x (0.0082 atm dm3 K-1 mol-1 x 358K)

    p x 3.47dm3 = 0.29 atm dm3

    p = (0.29 atm dm3 / 3.47 dm3)

    p = 0.085 atm

    Recall that pressure of the gas is required in mm hg, so convert 0.085 atm to mm Hg

    If 1 atm = 760 mm Hg

    0.085atm = 0.085 x 760

    = 64.6 mm Hg

    Thus, the pressure of the gas is 64.6 mm hg
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