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14 September, 20:05

What is the pressure of an ideal solution containing. 5 moles of a nonvolatile solute and 300g of ethanol at 40C? The vapor pressure of ethanol is 134 torr at 40C

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  1. 14 September, 22:33
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    The pressure of the solution is 144 torr

    Explanation:

    Step 1: Data given

    Number of moles of a nonvolatile solute = 0.5 moles

    Mass of ethanol = 300 grams

    Molar mass of ethanol = 46.07 g/mol

    Temperature = 40°C

    The vapor pressure of ethanol = 134 torr

    Step 2: Calculate moles ethanol

    Moles ethanol = mass ethanol / molar mass ethanol

    Moles ethanol = 300 grams / 46.07 g/mol

    Moles ethanol = 6.51 moles

    Step 3: Calculate the total moles

    Total moles = 0.5 moles + 6.51 moles

    Total moles = 7.01 moles

    Step 4: Calculate mol fraction

    Mol fraction = moles / total moles

    Mol fraction ethanol = 6.51 / 7.01 moles

    Mol fraction ethanol = 0.93

    Mol fraction nonvolatile solute

    0.5 moles / 7.01 moles = 0.07

    Step 5: Calculate Total pressure of the solution

    Vapor pressure ethanol = mol fraction * total pressure solution

    134 torr = 0.93 * total pressure solution

    Total pressure solution = 134 torr / 0.93

    Total pressure solution = 144 torr

    The pressure of the solution is 144 torr
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