Question

Calculate the quantity of heat gained or lost in the following change:

0.44 mol of water evaporates at 100 degrees Celsius

- So what I did was:

1 mol -> 6.01 kJ
0.44 mol -> x
x = 2.64 kJ of energy gained

But apparently this is incorrect? Could somebody please explain to me why and with the steps corrected? I might have a slight idea as to why it could be incorrect, like maybe the molar enthalpy of vaporization is not 6.01 kJ/mol. But then how would I know that value without researching this information? Thank you.

Answer 1

The heat of vaporization is 40.66 kJ/mol for water. I believe your 6.01 must be heat fusion for H2O.