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During lecture, there was a slide that mentioned that because heat is required during melting or boiling, the temperature of a sample remains constant even though heat is being added. Can someone please explain what this means?
I think this was in reference to the heating curves. My understanding is that if you to take the temperature of the boiling water it would remain the same temperature until there was a phase change even though you are continuing to add heat to the substance in order to induce said phase change.
I think this refers to the moment when a sample is about to change states of matter. If you observe a heat curve, you notice that when ice is melting into water or water is freezing into ice, temperature remains constant regardless of how much heat is added or lost. This is because the sample is absorbing all of the energy, causing its bond structures and abundance of certain intermolecular forces to change. But, it is only until it has absorbed or lost enough energy does the sample change temperature and states of matter.
To change something from one phase to another, say, solid to liquid, heat is needed. This can be easily seen in any real-life example (ice becoming water due to heat). What the slide means from "temperature staying constant" means that the process of adding heat is slow so the temperature manage to stay constant, despite the substance changing phases
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