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Assuming the mass of the ice in the beaker was 2000 g (2 kg), calculate the amount of heat that must have been added to convert the ice to water (assume that the entire 2000 g was ice at the start of melting, and the entire 2000 g was water at the end of the melting). Assume that the change took place entirely at 0 °C. The heat of fusion (DHfus) for H2O is 6.12 kJ/mol.

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Answer:

679.32 kJ

Explanation:

Heat required = number of moles * latent heat of fusion of water

So since we are given the mass of water and not the number of moles our first step is to calculate the number of moles of water available,

[tex]n = \frac{mass}{molar mass} = \frac{2000g}{18.01528g/mol}= 111.0 mol[/tex]

heat required = 111.0 mol * 6.12 kJ/mol

                       = 679.32 kJ

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