(a) How much heat must be removed to prepare 14.0 g of ice at 0.0^∘ C from 14.0 g of water at

step 1 So a liquid needs to release energy in order to reach a lower temperature as well as turn it int

(a) How much heat must be removed to prepare 14.0 g of ice...

(a) How much heat must be removed to prepare $14.0 \mathrm{~g}$ of ice at $0.0^{\circ} \mathrm{C}$ from $14.0 \mathrm{~g}$ of water at $25.0^{\circ} \mathrm{C} ?$ (b) Calculate the mass of water at $100.0^{\circ} \mathrm{C}$ that could be cooled to $23.5^{\circ} \mathrm{C}$ by the same amount of heat as that calculated in part (a).

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Key Concepts

Heat Transfer in Cooling Processes

Heat transfer in cooling processes involves removing energy from a substance to lower its temperature. This concept underpins calculations where the energy removed during cooling can be compared or equated to energy changes in other processes, such as phase changes or cooling from higher temperatures.

Sensible Heat

Sensible heat refers to the heat energy exchanged by a substance that results in a temperature change, as opposed to a phase change. It is calculated using the specific heat capacity, mass, and the temperature difference involved, and is critical for processes where the temperature is being lowered or raised without changing phase.

Latent Heat of Fusion

Latent heat of fusion is the energy needed to change a unit mass of a substance from the liquid phase to the solid phase (or vice versa) at a constant temperature. This concept is key when calculating the energy removal during a phase change, such as water freezing into ice.

Specific Heat Capacity

Specific heat capacity is the energy required to raise the temperature of a unit mass of a substance by one degree Celsius. It is essential for calculating the sensible heat change when a substance’s temperature changes while remaining in the same phase.

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