Given the following mixture of two compounds 20.00 mL of X (MW =99.00 g/mol)(density 0.918 g/mL) and 645.00 mL of Y (51.00 g/mol))(density 1.137 g/mL). The freezing point of pure Y is 90.00 degrees C. The molal freezing constant is 3.065 degrees C/m. What is the freezing point of the solution, in degrees C?
Given the following mixture of two compounds 20.00 mL of X (MW =99.00 g/mol)(density 0.918 g/mL) and 645.00 mL of Y (51.00 g/mol))(density 1.137 g/mL). The freezing point of pure Y is 90.00 degrees C. The molal freezing constant is 3.065 degrees C/m. What is the freezing point of the solution, in degrees C?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.95QE
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Given the following mixture of two compounds 20.00 mL of X (MW =99.00 g/mol)(density 0.918 g/mL) and 645.00 mL of Y (51.00 g/mol))(density 1.137 g/mL). The freezing point of pure Y is 90.00 degrees C. The molal freezing constant is 3.065 degrees C/m. What is the freezing point of the solution, in degrees C?
Given the following mixture of two compounds 35.00 mL of X (MW =80.00 g/mol)(density 0.945 g/mL) and 735.00 mL of Y (80.00 g/mol))(density 0.810 g/mL). The vapor pressure of pure Y is 47.00 torr. Calculate the vapor pressure of the solution.
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