Water boils at 100 degrees Celsius under normal conditions, but reducing the pressure lowers its boiling point; it may boil at 20 degrees Celsius. The lower the pressure, the lower the temperature required to boil.
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Of course, this may seem paradoxical, but it's a physical fact, not magic. Boiling depends on pressure as much as it does on temperature, as water molecules constantly transform into steam and then back into their liquid state. When water is heated, its vapor pressure increases. When this pressure equals the external pressure, the steam begins to form bubbles within the liquid, and the water boils.
It has been established that water boils at normal atmospheric pressure at sea level at a temperature of 100°C. However, this is not a fixed value. At an altitude of 2,000 meters, the atmospheric pressure is lower, and water boils at 93°C. On the summit of Everest, it boils at approximately 70°C. If the pressure surrounding the water decreases, its boiling point also decreases. At a pressure of approximately 2.3 kPa, water boils at 20°C, which is normal room temperature. This is confirmed by saturate vapor pressure data, as the vapor pressure of water at 20°C is approximately 2.33 kPa.
This phenomenon can be easily observed by placing a small amount of warm water in a syringe, then closing the opening with a finger and quickly pulling back the plunger. The pressure inside the syringe will then decrease, and the water will begin to boil, even though it remains at room temperature and has not been heated.
For a more visually clearer demonstration, a vacuum chamber is needed. Water at room temperature is placed under a glass lid, and the air is then evacuated. When the pressure drops to the saturation vapor pressure, the water begins to boil. This experiment is used in educational laboratories worldwide, as water boils when the pressure drops to the vapor pressure.
It's important to know that boiling water cools down quickly at room temperature because the steam carries away the heat, causing the water to cool. In a vacuum chamber, water can boil and then freeze; boiling and freezing can occur simultaneously. This is due to the water losing energy through evaporation.
Based on this, liquid water, if it existed on the surface of Mars, would boil almost instantly, given that the atmospheric pressure there is hundreds of times lower than on Earth. This is one reason why liquid water is unlikely to exist on the surface of Mars; water there tends to freeze or evaporate.
This problem becomes apparent when pumping fluids, as pumps create low-pressure areas, which can cause water to boil and steam bubbles to form. This phenomenon is known as cavitation, and when the bubbles collapse, they can damage the metal. Therefore, engineers take this phenomenon into account when designing pumps and pipelines.
Of course, we cannot observe water boiling under normal conditions at temperatures below 100 degrees Celsius because the changes in atmospheric pressure on Earth's surface are not significant enough. But in a vacuum chamber, inside a syringe, or on the surface of Mars, water can boil without the need for fire.
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