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    Convert the following pressure into atmospheres.
    781 torr
    781 mm Hg

    A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expnaded gas sample at a constant temperature.

    At conditions of constant temperature and pressure, the volume of a sample of ideal gas is proportional to the number of moles of gas present.

    If 3.25 mol of argon gas occupies a volume of 100L at a particular temperature and pressure, what volume does 14.15 mol of argon occupy under the same conditions.

    Suppose a 24.3-ml sample of helium gas at 25 degrees C and 1.01 atm is heated to 50 degrees C and compressed to a volume of 15.2 ml. What will the pressure of the sample be.

    © BrainMass Inc. brainmass.com December 24, 2021, 6:58 pm ad1c9bdddf
    https://brainmass.com/chemistry/gas-laws/application-ideal-gas-law-153560

    SOLUTION This solution is FREE courtesy of BrainMass!

    Please see the attached file.

    convert the following pressure into atmospheres.

    1. 1 torr = 1 mmHg
    1 atm = 760 mmHg
    So 1 mmHg = atm
    Then 781 torr = 781 mmHg = 781 * atm = 1.0276 atm

    2. A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L. What will be the pressure in the expnaded gas sample at a constant temperature.
    According to Boyle's law, at the constant temperature,

    At conditions of constant temperature and pressure, the volume of a sample of ideal gas is proportional to the number of moles of gas present.
    By ideal gas law,

    Where is constant with constant temperature and pressure.
    So V is directly proportional to the number of moles of the gas.

    If 3.25 mol of argon gas occupies a volume of 100L at a particular temperature and pressure, what volume does 14.15 mol of argon occupy under the same conditions.
    From the above equation, we know that with constant temperature and pressure:
    So

    The volume is 435.38 L.

    Suppose a 24.3-ml sample of helium gas at 25 degrees C and 1.01 atm is heated to 50 degrees C and compressed to a volume of 15.2 ml. What will the pressure of the sample be.
    By ideal gas law, is constant for certain moles of gas.
    The unit of the temperature T is Kelvin.
    So 25 C = 25 + 273.15 K
    50 C = 50 + 273.15 K

    The pressure is 1.75 atm.

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    © BrainMass Inc. brainmass.com December 24, 2021, 6:58 pm ad1c9bdddf>
    https://brainmass.com/chemistry/gas-laws/application-ideal-gas-law-153560

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