Calculate how much energy is required to heat 100 g of ice at 0 degrees Celsius to steam at 100 degrees Celsius.
Draw a diagram of temperature versus time for water being heated.
Heat of fusion of water = 6.02 kJ/ mole
Heat capacity of liquid water = 4.18 J/degree Celsius x g
Heat of vaporization of water = 40.7 kJ/ mole
** Please see the attached file for the diagram **
mass (m) = 100 g
initial state = ice
initial temperature (Ti) = 0 degrees C
final temperature (Tf) = 100 degrees C
final state = steam
Heat of fusion of water (Lf)= 6.02 kJ/ mole = 6.02*10^3 J/mole
1 mole of water = 18 ...
This solution goes through step-by-step calculations for the heat fusion of water to determine heat energy required. A diagram of time versus temperature is attached in a .jpg file.