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12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water. Calculate the theoretical freezing point of the mixture you created.

12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water. Calculate the theoretical freezing point of the mixture you created.

Chemistry
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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need help with #12
Imass of isopropanol (C3H§O). C =12.011 amu x3=36.033 amu H=1,008 annu x 8=8.064 amo = 60.096glmol O= 15,999 amu x 1=15.999 amu 9. Calculate the number of moles of isopropanol added to your ice solution. Pure isopropanol is 16.64 M. Molarity (o. of moles x I000) volume of solution no. of moles :(molaritysvol of sol.)/1000>C16.64 Mx 70 ml000 El.165 moles 10. Calculate the volume of water in your melted ice and isopropanol solution. Volume after ice melted - volume of Isopropanol 70-50=(20ml 11. Calculate the mass of water in the solution. (Recall that 1.0 mL of pure water has a mass of 1.0 g) Convert your answer to kg. Volume of isopropanol:50 m! Total volume of liquid in tumbler: 7oml Volume of uwater = 70-50 ml=20ml 20.0ml-20.0g → 20.og * 1 ha .02 ka 12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water. Calculate the theoretical freezing point of the mixture you created. 13. Compare the actual to the theoretical.
Transcribed Image Text:Imass of isopropanol (C3H§O). C =12.011 amu x3=36.033 amu H=1,008 annu x 8=8.064 amo = 60.096glmol O= 15,999 amu x 1=15.999 amu 9. Calculate the number of moles of isopropanol added to your ice solution. Pure isopropanol is 16.64 M. Molarity (o. of moles x I000) volume of solution no. of moles :(molaritysvol of sol.)/1000>C16.64 Mx 70 ml000 El.165 moles 10. Calculate the volume of water in your melted ice and isopropanol solution. Volume after ice melted - volume of Isopropanol 70-50=(20ml 11. Calculate the mass of water in the solution. (Recall that 1.0 mL of pure water has a mass of 1.0 g) Convert your answer to kg. Volume of isopropanol:50 m! Total volume of liquid in tumbler: 7oml Volume of uwater = 70-50 ml=20ml 20.0ml-20.0g → 20.og * 1 ha .02 ka 12. Recall that the freezing point is depressed by -1.86 °C per mole of solute per kg of water. Calculate the theoretical freezing point of the mixture you created. 13. Compare the actual to the theoretical.
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