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1 February, 11:14

An oxygen sample has a volume of 4.89 L at 27 °C and 800.0 torr. How many oxygen molecules does it contain?

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  1. 1 February, 13:42
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    For solving the question we use the ideal gas law:

    pressure * volume = moles * gas constant * temperature

    Because you have the pressure in torr the gas constant will have the following value:

    gas constant = 62.363 (L * torr) / (K * mol)

    To mach the unit of the constant the temperature have to be expressed in kelvin:

    T°K = T°C + 273

    T°K = 27 + 273 = 300 °K

    Now we add the values in the formula:

    pressure * volume = moles * gas constant * temperature

    800 * 4.89 = moles * 62.363 * 300

    moles = (800 * 4.89) / (62.363 * 300)

    moles = 0.209

    The we construct the following reasoning:

    if 1 mole of oxygen contains 6.022 * 10²³ molecules

    then 0.209 moles of oxygen contains X molecules

    X = (0.209 * 6.022 * 10²³) / 1 = 1.26 * 10²³ oxygen molecules
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