2) In an experiment to determine the molar mass of dichlorobenzens C6H4C12 using freezing point depression of solvent cyclohexane, a student uses 10 mL or cyclohexane (density 0.779 g/ ml) and obtains an average freezing point of 5.75 degrees Celsius. She graphically determines the new freezing point to be 2.8 degrees Celsius by setting equation of 2 lines equal to each other. What is her ATf? If she uses a total of 0.2301 grams of dichlorobenzene what is her calculated molecular weight for the solute? What is % error from actual molecular weight of solute? Is this a reasonable result?

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Chapter11: Properties Of Solutions
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2) In an experiment to determine the molar mass of dichlorobenzene C6H4C12 using freezing
point depression of solvent cyclohexane, a student uses 10 mL or cyclohexane (density 0.779 g/
ml) and obtains an average freezing point of 5.75 degrees Celsius. She graphically determines
the new freezing point to be 2.8 degrees Celsius by setting equation of 2 lines equal to each
other. What is her ATf? If she uses a total of 0.2301 grams of dichlorobenzene what is her
calculated molecular weight for the solute? What is % error from actual molecular weight of
solute? Is this a reasonable result?
Transcribed Image Text:× 2) In an experiment to determine the molar mass of dichlorobenzene C6H4C12 using freezing point depression of solvent cyclohexane, a student uses 10 mL or cyclohexane (density 0.779 g/ ml) and obtains an average freezing point of 5.75 degrees Celsius. She graphically determines the new freezing point to be 2.8 degrees Celsius by setting equation of 2 lines equal to each other. What is her ATf? If she uses a total of 0.2301 grams of dichlorobenzene what is her calculated molecular weight for the solute? What is % error from actual molecular weight of solute? Is this a reasonable result?
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