I have to design a lab to calculate the delta H value of the enthalpy change of ice to liquid water. It has to stay at 0*C
Needs to be in lab format but possible q=n(delta H) where n is the molarity
The Attempt at a Solution
I know the energy need to melt one mole of water is 6.02 KJ (oh so my Chem teacher tells me). I know that the energy need to heat up water increases until it hits 0*C then it plateaus until all the ice has melted, then it starts to increase again. What I'm not sure of is how to prove that the energy need is 6.02 KJ per mole.