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The equation `q = mΔH` is primarily used in chemistry and physics, specifically in the field of [thermodynamics](https://www.wikiwhat.page/kavramlar/thermodynamics), to calculate the heat absorbed or released during a **phase change**. Let's break down the components:
* `q`: Represents the [heat](https://www.wikiwhat.page/kavramlar/heat) energy transferred (absorbed or released), typically measured in Joules (J) or calories (cal).
* `m`: Represents the [mass](https://www.wikiwhat.page/kavramlar/mass) of the substance undergoing the phase change, usually measured in grams (g) or kilograms (kg).
* `ΔH`: Represents the [enthalpy%20change](https://www.wikiwhat.page/kavramlar/enthalpy%20change) of the phase transition. This is the amount of heat absorbed or released per unit mass of the substance during the phase change at constant pressure. It is often called the **latent heat** of the substance and is usually given in units of J/g or J/mol. Common specific names are the [enthalpy%20of%20fusion](https://www.wikiwhat.page/kavramlar/enthalpy%20of%20fusion) (melting or freezing) and the [enthalpy%20of%20vaporization](https://www.wikiwhat.page/kavramlar/enthalpy%20of%20vaporization) (boiling or condensation).
**Important Considerations:**
* This equation *only* applies during a phase change (e.g., melting, freezing, boiling, condensation, sublimation, deposition). During a phase change, the temperature remains constant.
* If the substance is being heated or cooled *without* a phase change, a different equation (`q = mcΔT`) is used.
* The sign of `ΔH` indicates whether the phase change is endothermic (heat absorbed, `ΔH` > 0) or exothermic (heat released, `ΔH` < 0).
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