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
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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