# How much heat must be removed to freeze a tray of ice cubes at 0 C if the water has a mass of 225 g?

Well, if the tray itself has a negligible heat capacity...

Hence, the amount of heat that is released at constant pressure is:

HINT: read the question wording again. Which direction is the heat flowing, and is the ice the system or surroundings?

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The amount of heat ( q ) required to freeze a substance can be calculated using the equation:

[ q = m \cdot \Delta H_f ]

Where:

- ( q ) is the heat absorbed or released (in joules)
- ( m ) is the mass of the substance (in grams)
- ( \Delta H_f ) is the heat of fusion (in joules per gram)

For water, the heat of fusion is ( 334 , \text{J/g} ).

Given that the mass of water is ( 225 , \text{g} ), and assuming the temperature change is from ( 0^\circ \text{C} ) to ( 0^\circ \text{C} ) during freezing, the heat required is:

[ q = 225 , \text{g} \times 334 , \text{J/g} = 75150 , \text{J} ]

So, ( 75150 , \text{J} ) of heat must be removed to freeze the tray of ice cubes.

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