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Based off information from the attachment, please help with #9 on second attachment

Based off information from the attachment, please help with #9 on second attachment

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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Based off information from the attachment, please help with #9 on second attachment
Procedure: Part I: Calibration step For best results, make some ice using distilled water. If that is not feasible, you can use ice made from tap water. However, realize that tap water does contain some solutes. Calibrate your thermometer. Fill a glass with ice. Add distilled water. Stir gently with the thermometer until the ice and water mixture has come to a stable temperature. Add more ice if most of the ice melts. You want to maintain a good mix of ice and water. It will probably take 10-15 minutes for the temperature to stabilize. Record the temperature to the nearest 0.1 degree. Measured temperature of pure ice water °C Recall that the melting point of water is 0.0 °C, so if your thermometer reads differently, you will need to adjust your temperature readings later in the experiment. For example, if your thermometer reads 0.5 °C in the plain ice water, and your solution reads -1.7 °C, then the actual difference in temperature between the two is -2.3 °C that 1.0 mL of pure water has a mass Part II: Isopropanol solution 1. Measure 50 mL of isopropanol (C3H3O). 2. Fill a tumbler with ice. Add the isopropanol. Add some distilled water. 3. Stir with the thermometer until a stable temperature is reached (this should be below 0 °C). This will probably take 10-15 minutes. 4. Record the lowest temperature observed; measure to the nearest 0.1 degree -\.2 °C 5. Adjust this temperature based on the calibration step as described above. Adjusted temperature_-2.0 °C 6. Let all of the ice melt, then measure the total volume of liquid in the tumbler/beaker. 70 mL
Transcribed Image Text:Procedure: Part I: Calibration step For best results, make some ice using distilled water. If that is not feasible, you can use ice made from tap water. However, realize that tap water does contain some solutes. Calibrate your thermometer. Fill a glass with ice. Add distilled water. Stir gently with the thermometer until the ice and water mixture has come to a stable temperature. Add more ice if most of the ice melts. You want to maintain a good mix of ice and water. It will probably take 10-15 minutes for the temperature to stabilize. Record the temperature to the nearest 0.1 degree. Measured temperature of pure ice water °C Recall that the melting point of water is 0.0 °C, so if your thermometer reads differently, you will need to adjust your temperature readings later in the experiment. For example, if your thermometer reads 0.5 °C in the plain ice water, and your solution reads -1.7 °C, then the actual difference in temperature between the two is -2.3 °C that 1.0 mL of pure water has a mass Part II: Isopropanol solution 1. Measure 50 mL of isopropanol (C3H3O). 2. Fill a tumbler with ice. Add the isopropanol. Add some distilled water. 3. Stir with the thermometer until a stable temperature is reached (this should be below 0 °C). This will probably take 10-15 minutes. 4. Record the lowest temperature observed; measure to the nearest 0.1 degree -\.2 °C 5. Adjust this temperature based on the calibration step as described above. Adjusted temperature_-2.0 °C 6. Let all of the ice melt, then measure the total volume of liquid in the tumbler/beaker. 70 mL
7. Calculate the volume of pure isopropanol in the 50 mL you measured, using the %. Recall that a % solution can be expressed as mL or g per 100 mL solution. 8. Calculate the molecular mass of isopropanol (C3H§O). C. = 12.011 amu x 3 =36.033 amu This ke many minutes Add H=1,008 annu x 8 = 8.064 amO- = 60.096gImol O= 15,999 amux 1:15.999 amu 9. Calculate the number of moles of isopropanol added to your ice solution. Pure isopropanol is 16.64 M. on your thmumeter calbeation. ru the volisne of solon to e ares 0.1ml 10. Calculate the volume of water in your melted ice and isopropanol solution. 9e the cheical us 20. e the molar 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. 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:7. Calculate the volume of pure isopropanol in the 50 mL you measured, using the %. Recall that a % solution can be expressed as mL or g per 100 mL solution. 8. Calculate the molecular mass of isopropanol (C3H§O). C. = 12.011 amu x 3 =36.033 amu This ke many minutes Add H=1,008 annu x 8 = 8.064 amO- = 60.096gImol O= 15,999 amux 1:15.999 amu 9. Calculate the number of moles of isopropanol added to your ice solution. Pure isopropanol is 16.64 M. on your thmumeter calbeation. ru the volisne of solon to e ares 0.1ml 10. Calculate the volume of water in your melted ice and isopropanol solution. 9e the cheical us 20. e the molar 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. 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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