The normal freezing point of a certain liquid X is -5.90 °C, but when 43. g of zinc chloride (ZnCl,) are dissolved in 400. g of X the solution freezes at -7.2 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. °C•kg Oxto K, mol ?
The normal freezing point of a certain liquid X is -5.90 °C, but when 43. g of zinc chloride (ZnCl,) are dissolved in 400. g of X the solution freezes at -7.2 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. °C•kg Oxto K, mol ?
Chapter2: The Kinetic Theory Of Gases
Section: Chapter Questions
Problem 70P: Using a numerical integration method such as Simpson's rule, find the fraction of molecules in a...
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