Question

Say that you have 54g sample of ice and you want to calculate the amount of heat energy that is required to melt that ice. (∆Hfus = 6kJ/mol) How much heat energy is required?​

Answer 1

First we have to change 54 g to mole=

(Ice = H2O)

54g * 1 mole of H2O/ 18.015 g

= 3 moles H2O

3 moles H2O= 3 moles ice

= 3 moles ice*6kj/mol / 1 mole ice

18 kj

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Answer 2

Answer:

Using the equation for a change in temperature and the value for water from Table 1, we find that Q = mLf = (1.0 kg)(334 kJ/kg) = 334 kJ is the energy to melt a kilogram of ice. This is a lot of energy as it represents the same amount of energy needed to raise the temperature of 1 kg of liquid water from 0ºC to 79.8ºC.