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Suppose a volatile liquid is completely vaporized into a 155 ml. flask in a 99.1°C bolling water bath. What is the molar mass of the volatileliquid if the corrected mass of the condensed vapor is 0.207 g and the final partial pressure of air in the flask is 687 mm Hg? Туре аnswer:

Suppose a volatile liquid is completely vaporized into a 155 ml. flask in a 99.1°C bolling water bath. What is the molar mass of the volatileliquid if the corrected mass of the condensed vapor is 0.207 g and the final partial pressure of air in the flask is 687 mm Hg? Туре аnswer:

Introductory Circuit Analysis (13th Edition)
Introductory Circuit Analysis (13th Edition)
13th Edition
ISBN:9780133923605
Author:Robert L. Boylestad
Publisher:Robert L. Boylestad
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Certainly! Here is the transcribed text for the educational website: --- **Problem Statement:** Suppose a volatile liquid is completely vaporized into a 155 mL flask in a 99.1°C boiling water bath. What is the molar mass of the volatile liquid if the corrected mass of the condensed vapor is 0.207 g and the final partial pressure of air in the flask is 687 mm Hg? **Type answer:** [Text box for answer entry] --- **Explanation:** To solve this problem, use the Ideal Gas Law equation: \[ PV = nRT \] Where: - \( P \) is the pressure (in atm), - \( V \) is the volume (in liters), - \( n \) is the number of moles, - \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), - \( T \) is the temperature (in Kelvin). **Steps:** 1. Convert the temperature to Kelvin: - \( T = 99.1°C + 273.15 = 372.25 \, K \) 2. Convert the volume from mL to L: - \( V = 155 \, mL = 0.155 \, L \) 3. Convert the pressure from mm Hg to atm: - \( P = \frac{687 \, mmHg}{760 \, mmHg/atm} \approx 0.904 \, atm \) 4. Find the number of moles \( n \) using the Ideal Gas Law: - \( n = \frac{PV}{RT} \) 5. Calculate the molar mass: - Molar mass = \(\frac{{\text{mass of the vapor}}}{{n}}\) Using these steps, you can find the molar mass of the volatile liquid. --- If diagrams or graphs were present, they would be explained here in detail regarding their features, axes, labels, and any significant data points.
Transcribed Image Text:Certainly! Here is the transcribed text for the educational website: --- **Problem Statement:** Suppose a volatile liquid is completely vaporized into a 155 mL flask in a 99.1°C boiling water bath. What is the molar mass of the volatile liquid if the corrected mass of the condensed vapor is 0.207 g and the final partial pressure of air in the flask is 687 mm Hg? **Type answer:** [Text box for answer entry] --- **Explanation:** To solve this problem, use the Ideal Gas Law equation: \[ PV = nRT \] Where: - \( P \) is the pressure (in atm), - \( V \) is the volume (in liters), - \( n \) is the number of moles, - \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), - \( T \) is the temperature (in Kelvin). **Steps:** 1. Convert the temperature to Kelvin: - \( T = 99.1°C + 273.15 = 372.25 \, K \) 2. Convert the volume from mL to L: - \( V = 155 \, mL = 0.155 \, L \) 3. Convert the pressure from mm Hg to atm: - \( P = \frac{687 \, mmHg}{760 \, mmHg/atm} \approx 0.904 \, atm \) 4. Find the number of moles \( n \) using the Ideal Gas Law: - \( n = \frac{PV}{RT} \) 5. Calculate the molar mass: - Molar mass = \(\frac{{\text{mass of the vapor}}}{{n}}\) Using these steps, you can find the molar mass of the volatile liquid. --- If diagrams or graphs were present, they would be explained here in detail regarding their features, axes, labels, and any significant data points.
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