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8 October, 22:49

How many grams of CO2 or an 800 mL at 94.5 K PA at - 10°C?

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  1. 8 October, 22:50
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    1.52g

    Explanation:

    First, let us calculate the number of mole of CO2 present. This is illustrated below:

    V = 800mL

    Recall: 1000mL = 1L

    800mL = 800/1000 = 0.8L

    P = 94.5 KPa = 94500Pa

    Recall: 101325Pa = 1atm

    94500Pa = 94500/101325 = 0.93atm

    T = - 10°C = - 10 + 273 = 263K

    R = 0.082atm. L/Kmol

    n = ?

    PV = nRT

    n = PV/RT

    n = (0.8x0.93) / (0.082x263)

    n = 0.0345mol

    Now, we can obtain the mass of CO2 as follows:

    Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

    Number of mole of CO2 = 0.0345mol

    Mass of CO2 = number of mole x molar Mass

    Mass of CO2 = 0.0345 x 44 = 1.52g
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