# The normal boiling point of water is 100 Celcius and

The normal boiling point of water is 100 Celcius and the molar enthalpy of vaporization of water is 40.7 KJ/mol. What is the boiling point of water under a pressure of 0.500 atm?
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empatteMattmkezo
Given,
The normal boiling point of water $\left({T}_{1}\right)={100}^{\circ }C=\left(273.15+100K\right)=373.15K$
Note: pressure at normal boiling point of water
Boiling point of water under a pressure of 0.500 atm $\left({T}_{2}\right)=?$
Pressure $\left({P}_{2}\right)=0.500$
Molar enthalpy of vaporization
Note: universal gas constant
Calculating the boiling point of water under a pressure of 0.500 atm $\left({T}_{2}\right)$:

Conclusion,
So, the boiling point of water under a pressure of 0.500 atm is ${81.26}^{\circ }C$
Answer: ${81.26}^{\circ }C$