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13 September, 07:23

The nonvolatile, nonelectrolyte DDT, C14H9Cl5 (354.50 g/mol), is soluble in diethyl ether CH3CH2OCH2CH3. Calculate the osmotic pressure generated when 10.4 grams of DDT are dissolved in 286 ml of a diethyl ether solution at 298 K. The molarity of the solution is M. The osmotic pressure of the solution is atmospheres.

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  1. 13 September, 07:32
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    2.50 atm

    Explanation:

    We have 10.4 g of DDT (solute), whose molar mass is 354.50 g/mol. The corresponding moles are:

    10.4 g * (1 mol/354.50 g) = 0.0293 mol

    The molarity of the solution is:

    M = moles of solute / liters of solution

    M = 0.0293 mol / 0.286 L

    M = 0.102 M

    We can find the osmotic pressure (π) using the following pressure.

    π = M * R * T

    where,

    R: ideal gas constant

    T: absolute temperature

    π = M * R * T

    π = 0.102 M * 0.0821 atm. L/mol. K * 298 K

    π = 2.50 atm
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