ThermodynamicsHard

Question

The heat capacity of liquid water is 75.6 J/K-mol, while the enthalpy of fusion of ice is 6.0 kJ/mol. What is the smallest number of ice cubes at 0°C each containing 9.0 g of water needed to cool 500 g of liquid water from 20°C to 0°C?

Options

A.1
B.7
C.14
D.21

Solution

Heat lost by water = Heat gained by ice

$\text{Or, 500} \times \frac{75.6}{18} \times 20 = (N \times 9) \times \frac{6000}{18} \Rightarrow N = 14$

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