A nitrogen oxide contains 30.4% N and 69.6% O and has a mass of 0.66g when vaporized in 225 ml flask at 100 degree C and atmospheric pressur?

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  • Dr W
    Lv 7
    2 months ago

    assuming it's an ideal gas

    .. PV = nRT

    .. PV = (mass / mw) RT

    .. mw = mass * RT / (PV)

    solve for molar mass.. mw

    .. mw = 0.66g * (0.08206 Latm/molK) * (373,15K) / (1atm * 0.225L) = __g/mol

    then assume 1 mole NOx

    .. mol N = __g NOx * (0.304g N / 1g NOx) * (1 mol N / 14.01g N) = __ mol N

    .. mol O = __g NOx * (0.696g O / 1g NOx) * (1 mol O / 16.00g O) = __ mol O

    and there you go... just fill in the blanks

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