**Determining the Molar Mass of a Volatile Liquid****Procedure Summary:**This experiment describes a method for determining the molar mass of a volatile liquid using a syringe. Here's an overview of the process:1. A liquid with a mass of 0.0152 grams is placed into a syringe, which is then sealed by capping the end.2. The syringe is submerged in a temperature bath set at 45.3°C, causing the liquid to vaporize.3. As the liquid vaporizes, it expands and pushes the plunger outward.4. Once equilibrium is reached, the volume of the gas is measured at 4.79 mL.5. Atmospheric pressure during this experiment is recorded as 740 mmHg.**Objective:**The aim is to calculate the approximate molar mass of the compound (in g/mol). **Instructions:**Use the provided measurements and conditions to determine the molar mass. Note the hint provided in the feedback for additional guidance.**Response Box:**An answer box is available for students to input their calculated molar mass. **Note:** There are no graphs or diagrams included in this description.

Given, Mass of liquid = 0.0152 g Temperature = 45.3◦c Volume = 4.79 mL Pressure = 740 mm Hg

The following procedure provides a crude method of determining the molar màss of a volatile liquid. A liquid of mass 0.0152 g is introduced into a syringe and the end is capped (sealed). The syringe is transferred to a temperature bath maintained at 45.3 °C, and the liquid vaporizes. As the liquid vaporizes the plunger is pushed out. At equilibrium, the plunger reads 4.79 mL of gas. Atmospheric pressure is 740. mmHg. What is the approximate molar mass of the compound (in g/mol)? Hint is given in the feedback. Answer:

The following procedure provides a crude method of determining the molar màss of a volatile liquid. A liquid of mass 0.0152 g is introduced into a syringe and the end is capped (sealed). The syringe is transferred to a temperature bath maintained at 45.3 °C, and the liquid vaporizes. As the liquid vaporizes the plunger is pushed out. At equilibrium, the plunger reads 4.79 mL of gas. Atmospheric pressure is 740. mmHg. What is the approximate molar mass of the compound (in g/mol)? Hint is given in the feedback. Answer:

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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