The normal freezing point of a certain liquid x is -6.20 °C, but when 36. g of iron(III) chloride (FeCl,) are dissolved in 300. g of x the solution freezes at -9.4 °C instead. Use this information to calculate the molal freezing point depression constant K, of x. Round your answer to 2 significant digits. °C · kg K, = 0- mol ?
The normal freezing point of a certain liquid x is -6.20 °C, but when 36. g of iron(III) chloride (FeCl,) are dissolved in 300. g of x the solution freezes at -9.4 °C instead. Use this information to calculate the molal freezing point depression constant K, of x. Round your answer to 2 significant digits. °C · kg K, = 0- mol ?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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![The normal freezing point of a certain liquid x is -6.20 °C, but when 36. g of
iron(III) chloride (FeCl,) are dissolved in 300. g of x the solution freezes at
-9.4 °C instead. Use this information to calculate the molal freezing point
depression constant K, of x.
Round your answer to 2 significant digits.
do
°C · kg
K, = 0-
mol
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8dd7c44c-daf0-47b5-9af2-540ecc18f39f%2F8cb82869-50c3-4f1e-80e8-f80dec32ca3d%2F5ej57jr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The normal freezing point of a certain liquid x is -6.20 °C, but when 36. g of
iron(III) chloride (FeCl,) are dissolved in 300. g of x the solution freezes at
-9.4 °C instead. Use this information to calculate the molal freezing point
depression constant K, of x.
Round your answer to 2 significant digits.
do
°C · kg
K, = 0-
mol
?
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