(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 in this question, we are going to calculate the heat that has to be removed to prepare 14 gra

(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 $25.0^{\circ} \mathrm{C}^{2}$ (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

Latent Heat of Fusion

Latent heat of fusion is the amount of energy per unit mass needed to change a substance from a liquid to a solid (or vice versa) without a change in temperature. This is crucial when calculating the energy required to freeze water at 0°C, since even though the temperature remains constant, a significant amount of heat must be removed to accomplish the phase change.

Calorimetry

Calorimetry is the measurement of the amount of heat exchanged in physical and chemical processes. It combines the concepts of specific heat and latent heat to determine the overall energy balance in processes like cooling, heating, and phase changes, ensuring the conservation of energy within the system.

Specific Heat Capacity

This concept refers to the amount of heat required to change the temperature of a unit mass of a substance by one degree Celsius (or Kelvin). It is key in calculating how much energy is removed or added when a substance, like water, is heated or cooled over a temperature range, as seen in determining the energy change from 25°C to 0°C or from 100°C to 23.5°C.

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