* Atmospheric Pressure: The boiling point of a liquid is the temperature at which its vapor pressure equals the surrounding atmospheric pressure. At higher altitudes, the atmospheric pressure is lower.
* Lower Pressure, Lower Boiling Point: Since the pressure on the water is lower on a mountain, it takes less energy for the water molecules to escape into the air as vapor. This means the water boils at a lower temperature.
Think of it this way:
Imagine you're trying to pop a balloon. If you're at a high altitude, where the air pressure is lower, it's easier to pop the balloon because there's less pressure pushing back. Similarly, water molecules at higher altitudes experience less pressure, making it easier for them to "pop" into the air as vapor.
Example:
Water boils at 100°C (212°F) at sea level. But on Mount Everest, where the atmospheric pressure is much lower, water boils at around 70°C (158°F).
