**Determining the Vapor Pressure of an Unknown Liquid****Problem Statement:**An unknown liquid has a heat of vaporization of 31.32 kJ/mole. If the normal boiling point is 88°C, what is the vapor pressure (in torr) of this liquid at room temperature of 25°C? **Hint:**Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).**Explanation:**To solve this problem, we use the Clausius-Clapeyron equation which relates the vapor pressure of a substance at two different temperatures. The Clausius-Clapeyron equation can be written as:\[ \ln \left( \frac{P_2}{P_1} \right) = - \frac{\Delta H_\text{vap}}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right) \]Where: - \( P_1 \) is the initial vapor pressure (760 mm Hg at the boiling point).- \( P_2 \) is the vapor pressure at the new temperature.- \( \Delta H_\text{vap} \) is the heat of vaporization (31.32 kJ/mole).- \( R \) is the ideal gas constant (8.314 J/mol·K).- \( T_1 \) is the initial temperature in Kelvin (88°C = 361 K).- \( T_2 \) is the new temperature in Kelvin (25°C = 298 K). Solve for \( P_2 \):1. Convert the heat of vaporization from kJ/mole to J/mole:\[ \Delta H_\text{vap} = 31.32 \text{ kJ/mole} \times 1000 \text{ J/kJ} = 31320 \text{ J/mole} \]2. Substitute the values into the Clausius-Clapeyron equation:\[ \ln \left( \frac{P_2}{760 \text{ mm Hg}} \right) = - \frac{31320 \text{ J/mole}}{8.314 \text{ J/mol·K}} \left( \frac{1}{298 \text{ K}} - \frac{1}{361 \text{ K}} \

T he normal boiling point is the temperature at standard atmospheric pressure that is 760 mmHg.…

An unknown liquid has a heat of vaporization of 31.32 kJ/mole. If the normal boiling point is 88, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

An unknown liquid has a heat of vaporization of 31.32 kJ/mole. If the normal boiling point is 88, what is vapor pressure (in torr) of this liquid at room temperature of 25 degrees C? HINT: Normal boiling point occurs when the vapor pressure of the liquid is the same as atmospheric pressure (1 atm or 760 mm Hg).

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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