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12 September, 03:28

How much water would be needed to completely dissolve 1.78 L of the gas at a pressure of 735 torr and a temperature of 24 ∘C?

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  1. 12 September, 04:00
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    Answer: 0.46L

    Explanation:

    KH = 0.158mol/L/atm

    Pg = 735 torr = 735/760 = 0.967atm

    C=?

    C = KH x Pg = 0.158 x 0967

    C = 0.153mol/L

    T = 24°C = 24 + 273 = 297K

    R = 0.082atm. L/K/mol

    P = 0.967atm

    V = 1.78 L

    n=?

    PV = nRT

    n = PV / RT = (0.967x1.78) / (0.082x297)

    n = 0.071mol

    0.153mol dissolves in 1L of water. therefore, 0.071mol will dissolve in = 0.071/0.153 = 0.46L
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