Why does heavy water (D2O) boil at 101.42° C compared to 100°C of regular water?
I've heard two explanations for this, and I can't remember which one is correct: one is that that because a molecule of D2O is heavier than a molecule of H2O, it takes more energy, i.e. higher temperature, to boil. The other is that there are stronger Hydrogen bonds in D2O compared to H2O.
I'll look into it.
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I was late for work this morning, because I got stuck in Zeno's paradox.
As far as I know, Tom's second explanation is the correct one. Water is composed of 2 hydrogen atoms connected to an oxygen atom. The water molecules are connected to one another via hydrogen bonds. Deuterium is hydrogen which contains an extra neutron, and therefore the hydrogen bonds that it forms are stronger and more energy is needed to break them.
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