You're heating a pot of water on the stove. The water reaches 100°C and starts boiling vigorously. You turn the burner to maximum.
What happens to the water's temperature while it's boiling?
The temperature stays at 100°C the ENTIRE time it's boiling! All that extra heat energy goes into breaking bonds between water molecules, not making them hotter.
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Watch the temperature graph as you heat ice through water to steam. Notice the FLAT plateaus at 0°C and 100°C — that's latent heat at work.
Q = mL
It takes 7× more energy to boil water than to heat it from 0°C to 100°C!
Ice cools your drink by absorbing 334 J/g while melting — that's why ice water stays cold so long
Steam at 100°C causes worse burns than water at 100°C — it releases 2,260 J/g of latent heat on contact
Hurricanes are powered by latent heat — water vapor releasing enormous energy when it condenses into rain
“Phase transitions are nature's energy storage — hidden in bonds, invisible in temperature.”
Heating Curve
Heat a substance from solid through liquid to gas. Watch the temperature plateaus and see molecular behavior change at each transition.
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Heat the substance slowly and count how long the temperature stays flat at each transition. Which phase change uses more energy — melting or boiling?
Boiling requires about 7× more energy than melting for water. This is because gas molecules must completely separate, while liquid molecules just need to break their rigid lattice structure.