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3. Calculate the average molar mass from your three trials. Calculate the standard deviation in your value for molar mass. (See the popcorn experiment for the equation)

3. Calculate the average molar mass from your three trials. Calculate the standard deviation in your value for molar mass. (See the popcorn experiment for the equation)

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
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I need help with question 3. The answers to question 2 is above the questions.  

Procedure You are given an UNKNOWN VOLATILE LIQUID. You put 5 mL in a weighed flask tightly capped with a piece of aluminum foil with a pinhole. This is heated in a boiling water bath, until the vapors completely displace all the air, and all of the liquid has evaporated. The pin is replaced. The flask is then cooled to recondense the vapors and weighed. The exact volume of the flask is also determined. Data Atmospheric pressure 23.94 inch Hg Trial Water Initial mass of Final mass of Volume of the flask, pin and foil (g) Erlenmeyer Flask (mL) flask, foil, pin and Temperature (degrees Celsius) recondensed volatile liquid (g) 83.15g 83.24g 83.3g 83.79g 84.23g 84.02g 146mL 95 C 148mL 3 95 C 147mL Avg. 147mL Questions 2. Average volume =147 mL And molar mass from each trial is- Trial 1, molar mass = 164.37 g/mol, Trial 2: Molar mass =254.26 g/mol, Trial 3: Molar mass = 184.92 g/mol 2. Calculate the average volume of the flask using the data from your three measurements. Use this average value to calculate the molar mass of your volatile liquid for each of your three trials of mass determination. (Don't forget to convert your temperature to the absolute scale.) 3. Calculate the average molar mass from your three trials. Calculate the standard deviation in your value for molar mass. (See the popcorn experiment for the equation) 4. Explain why the pin must be replaced into the pinhole during cooling of the flask. 5. Due to the fact that the liquid you used was a volatile one, it will not completely recondense. Some of the liquid remains in the vapor phase, even at room temperature. If you were able to correct for this by making the vapors recondense completely, would your final molar mass value be greater than, less than or the same as the value you determined? Explain your reasoning.
Transcribed Image Text:Procedure You are given an UNKNOWN VOLATILE LIQUID. You put 5 mL in a weighed flask tightly capped with a piece of aluminum foil with a pinhole. This is heated in a boiling water bath, until the vapors completely displace all the air, and all of the liquid has evaporated. The pin is replaced. The flask is then cooled to recondense the vapors and weighed. The exact volume of the flask is also determined. Data Atmospheric pressure 23.94 inch Hg Trial Water Initial mass of Final mass of Volume of the flask, pin and foil (g) Erlenmeyer Flask (mL) flask, foil, pin and Temperature (degrees Celsius) recondensed volatile liquid (g) 83.15g 83.24g 83.3g 83.79g 84.23g 84.02g 146mL 95 C 148mL 3 95 C 147mL Avg. 147mL Questions 2. Average volume =147 mL And molar mass from each trial is- Trial 1, molar mass = 164.37 g/mol, Trial 2: Molar mass =254.26 g/mol, Trial 3: Molar mass = 184.92 g/mol 2. Calculate the average volume of the flask using the data from your three measurements. Use this average value to calculate the molar mass of your volatile liquid for each of your three trials of mass determination. (Don't forget to convert your temperature to the absolute scale.) 3. Calculate the average molar mass from your three trials. Calculate the standard deviation in your value for molar mass. (See the popcorn experiment for the equation) 4. Explain why the pin must be replaced into the pinhole during cooling of the flask. 5. Due to the fact that the liquid you used was a volatile one, it will not completely recondense. Some of the liquid remains in the vapor phase, even at room temperature. If you were able to correct for this by making the vapors recondense completely, would your final molar mass value be greater than, less than or the same as the value you determined? Explain your reasoning.
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