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12 July, 17:33

A 0.6-m3 rigid tank contains 0.6 kg of N2 and 0.4 kg of O2 at 300 K. Determine the partial pressure of each gas and the total pressure of the mixture. The gas constant for N2 is 0.2968 kPa·m3/kg·K and the gas constant for O2 is 0.2598 kPa·m3/kg·K.

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  1. 12 July, 17:54
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    Pnitrogen=3.18 kPa, Poxygen=1.62 kPa, Ptotal = 4.80 kPa

    Explanation:

    partial pressure equation becomes Ptotal = Pnitrogen + Poxygen

    Partial pressure of Nitrogen

    Pnitrogen = nRT/V

    n=no of moles = mass/molar mass

    mass of nitrogen=0.6kg

    Molar mass of nitrogen gas=28gmol^-1

    n=0.6/28=0.0214moles

    R=0.2968 kPa·m3/kg·K

    T=300k

    V=0.6m^3

    Pnitrogen = (0.0214 * 0.2968 * 300) / 0.6

    Pnitrogen=3.18 kPa

    Likewise

    Poxygen=nRT/V

    n=0.4/32=0.0125moles

    R=0.2598 kPa·m3/kg·K

    T=300k

    V=0.6m^3

    Poxygen = (0.0125 * 0.2598 * 300) / 0.6

    Poxygen=1.62 kPa

    Ptotal = 3.18+1.62 = 4.80 kPa
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