The equilibrium vapor pressure of the liquid of a pure substance becomes doubled when the temperature is raised from 25.4 °C to 37.2 °C. Determine the molar enthalpy of vaporization in units of kJ/mol with 3 significant figures. Type in only the number. Blackboad does not recognize units.
The equilibrium vapor pressure of the liquid of a pure substance becomes doubled when the temperature is raised from 25.4 °C to 37.2 °C. Determine the molar enthalpy of vaporization in units of kJ/mol with 3 significant figures. Type in only the number. Blackboad does not recognize units.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Transcribed Image Text:The equilibrium vapor pressure of the liquid of a pure substance becomes doubled when the temperature is raised
from 25.4 °C to 37.2 °C. Determine the molar enthalpy of vaporization in units of kJ/mol with 3 significant figures. Type
in only the number. Blackboad does not recognize units.
Expert Solution
Step 1
Given data is as follows:
The equilibrium vapor pressure of the substance = P
The pressure becomes when temperature changes = 2P
The molar enthalpy of vaporization
Step by step
Solved in 2 steps
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