An ice-cube tray of negligible mass contains 0.350 kg of water at 18.0^∘ C . How much heat must

step 1 In this problem, we have a temperature change and we have a phase change from liquid to solid. S

An ice-cube tray of negligible mass contains 0.350 kg of...

An ice-cube tray of negligible mass contains 0.350 $\mathrm{kg}$ of water at $18.0^{\circ} \mathrm{C}$ . How much heat must be removed to cool the water to $0.00^{\circ} \mathrm{C}$ and freeze it? Express your answer in joules, calories, and Btu.

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Key Concepts

Phase Change

Phase change is the process of a substance changing its state, such as from liquid to solid or vice versa, which involves latent heat. During this process, energy is absorbed or released without a change in temperature, distinguishing it from heating or cooling within a single phase.

Unit Conversions

Unit conversions are necessary to express physical quantities like heat energy in different measurement systems, such as joules, calories, or Btu. This involves using established conversion factors to translate a value in one unit to equivalent values in other units, ensuring consistency and comparability of results.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise or lower the temperature of a unit mass of a substance by one degree Celsius. It is a key property in calculating the energy needed for temperature changes without a phase change, involving the formula Q = m*c*?T, where m is mass, c is specific heat, and ?T is the change in temperature.

Latent Heat of Fusion

Latent heat of fusion refers to the heat energy required per unit mass to change a substance from a solid to a liquid or vice versa at its melting/freezing point without changing its temperature. This concept is essential for calculating the energy removal or addition during the phase change process, represented by Q = m*Lf.

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