Chemistry

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What is the pressure, in torr, of a gas whose density is 8.0 g/L at a temperature of 25 C above standard temperature and whose molecular weight is 75 g/mol?

  • Chemistry -

    Use the gas law and solve for the pressure:

    PV=nRT

    Where

    n=moles of gas
    L=volume
    R=62.3637 L·Torr/mol·K
    and
    T=273.15K + 25 C=298.15K

    The density of the gas is 8.0g/L and the molecular weight of the gas is 75 g/mol

    8.0g//75g/mol= x mol/L

    Rearrangement of the gas law gives the following:

    P=(n/V)*RT


    Plug in x mol/L into the equation and plug and chug.

  • Chemistry-Typo Fix -

    **Fixed a typo that probably would cause confusion.

    Use the gas law and solve for the pressure:

    PV=nRT

    Where

    n=moles of gas
    L=volume
    R=62.3637 L·Torr/mol·K
    and
    T=273.15K + 25 C=298.15K

    The density of the gas is 8.0g/L and the molecular weight of the gas is 75 g/mol

    8.0g/L**/75g/mol= x mol/L

    ***This leaves mol/L

    Rearrangement of the gas law gives the following:

    P=(n/V)*RT


    Plug in x mol/L into the equation and plug and chug.

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