Boiling happens when a liquid’s vapor pressure matches the atmospheric pressure around it. Think of it as the liquid screaming, “Let me out!” until the air pressure finally gives in. The stronger the intermolecular forces in that liquid, the harder it has to scream—meaning a higher temperature to boil.
Here’s the kicker: not all liquids are equal. Water has hydrogen bonds—those clingy little hugs between molecules. Oil? Just weak van der Waals forces—they’re like lazy handshakes. Water wins: 100°C vs. oil’s 150-300°C. Crazy, right?
Water vs. Ethanol: The Classic Showdown
You’ve seen this in the kitchen. A splash of vodka on a hot pan sizzles away immediately. Ethanol boils at a mere 78°C. Water? It’s a stubborn mule at 100°C. Why? Ethanol is a bit of a loner—its molecules don’t stick together as tightly as water’s do.
So next time you’re making pasta, that little steam dance? It’s water’s hydrogen bonds throwing a party at 100°C. Ethanol would have evaporated before you even dropped the spaghetti. (Yes, I just compared pasta to vodka. Deal with it.)
