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21 July, 21:24

What is the density of CO2 at a pressure of 0.0079 atm and 227 K? (These are the approximate atmospheric in Mars)

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  1. 21 July, 21:44
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    The density is 0.0187 g/L

    Explanation:

    First thing to do here is to calculate the Volume of 1 mole of CO2 using the ideal gas equation

    Mathematically;

    PV = nRT

    thus V = nRT/P

    what we have are;

    n = 1 mole

    R is the molar has constant = 0.082 L•atm•mol^-1•K^-1

    P is the pressure = 0.0079 atm

    T is temperature = 227 K

    Substituting these values, we have;

    V = nRT/P = (1 * 0.082 * 227) / 0.0079

    V = 2,356.20 dm^3

    This means according to the parameters given in the question, the volume of 1 mole of carbon iv oxide is 2,356.20 dm^3

    But this is not what we want to calculate

    What we want to calculate is the density

    Mathematically, we can calculate the density using the formula below;

    density = molar mass/molar volume

    Kindly recall that the molar mass of carbon iv oxide is 44 g/mol

    Thus the density = 44/2356.20 = 0.018674136321195 which is approximately 0.0187 g/L
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