10.2234 kJ of heat is needed to completely melt 1.70 moles of H2O, given that the water is at its melting point and the heat of fusion for water is 6.02 kJ/mole.
What is latent heat?
The term "latent heat" refers to the heat energy that a substance retains when its phase changes during a specific process. The latent heat of evaporation, which occurs when a liquid absorbs heat from an external source at its boiling point, is one of many types of latent heat.
Similarly, the latent heat of fusion is used when any substance melt at its melting point to change the liquid phase of that substance.
As given in the problem, The heat of fusion for water is 6.02 kJ/mole. This means 6.02 kJ heat is needed to melt 1 mole of ice into water
Then the heat are needed to completely melt 1.70 moles of H2O,
Heat = 1.70 moles ×6.02 kJ/mole
Heat = 10.2234 kJ
Thus, the heat needed to completely melt 1.70 moles of H2O is 10.2234 kJ
Learn more about Latent heat from here
brainly.com/question/13428994
#SPJ2
