The molar heat of vaporization of water is 40.7kJ/mol. How much heat must be absorbed to convert 50.0 grams of liquid water at 100oC to steam at 100oC?
A) 1.46 X 10 kJ
B) 1.13 X 102kJ
C) 2.04 X 103kJ
D) 3.66 X 104kJ

Question

The molar heat of vaporization of water is 40.7kJ/mol. How much heat must be absorbed to convert 50.0 grams of liquid water at 100oC to steam at 100oC?
A)	1.46 X 10 kJ	
B)	1.13 X 102kJ	
C)	2.04 X 103kJ	
D)	3.66 X 104kJ

littleredriding · Answer

@Photon336

frostbite · Answer

In a phase transition you simply multiply your amount of substance onto the molar heat of ???

So in this case you simply find the amount of mol of water and then multiply it with you molar heat of vaporization. I can check your answer in a little while.

sweetburger · Answer

q=mc
Delta T is non-existant
convert your 50grams of H2O to moles