# Question #2ca27

##### 1 Answer

#### Explanation:

In order to be able to answer this question, you need to know the value of the **enthalpy of vaporization** of water

#DeltaH_"vap" = "2257 J g"^(-1)#

https://en.wikipedia.org/wiki/Enthalpy_of_vaporization

The enthalpy of vaporization tells you the energy needed to convert

In this case, you know that in order to convert

You can use the **molar mass** of water to determine the *molar enthalpy of vaporization*, which represents the energy needed to convert **mole** of water from liquid at

#18.015color(white)(.)color(red)(cancel(color(black)("g")))/"mol" * "2257 J"/(1color(red)(cancel(color(black)("g")))) = "40,660 J mol"^(-1)#

This means that in order to convert **mole** of water, at its normal boiling point to vapor at

#"40,660 J " = " 40.66 kJ"#