What is the boiling point of water

Once water starts boiling, its temperature remains stable. Do you know what happens to the temperature of water boiling in a pot on high heat? It’s a common science question, particularly for tests, because knowing the answer shows how well you understand the process of boiling. The answer is the The temperature at which water boils isn’t the same everywhere. Boiling point depends on pressure. At sea level, water boils at 100 °C (212 °F) and freezes at 0 °C (32 °F). If you boil water at a higher pressure (below sea level, for example), the But, whatever the boiling point is, when water reaches it and undergoes a phase transition into water vapor (steam), the temperature stops rising. You can crank the heat as high as you like. The water may boil more vigorously and convert into steam more quickly, but it won’t get hotter. In fact, at the microscopic level, there may be cooler regions of boiling water. When vapor bubbles form near a heat source, like at the bottom of a pot, the gas bubbles insulate the water from the heat. It’s not a big deal for home cooking, but is an important consideration for industrial applications. Water Hotter Than Boiling Point and Colder Than Freezing Point Liquid water can be hotter than100 °C (212 °F) and colder than 0 °C (32 °F). Heating water above its boiling point without boiling is called superheating. If water is superheated, it can exceed its boiling point without boiling. You may have firsthand experience with the phenomenon, as its fair...

The boiling point of water is $\pu$. At what temperature, can you say for certain that all water vapor will turn into liquid? In other words, what is the condensation point of water? $\begingroup$ If I'm not mistaken that is technically not right (although this is more semantics than anything else). Once water has become ice (under normal condition $<0^o$C), the process of ice turning into gas is not evaporation but sublimation. So below freezing there is no evaporation. $\endgroup$ You're right - water vapor can exist at temperatures such as $\pu$, but rather the average exists at that temperature. To answer your question, never in a real scenario. From a chemical engineering perspective (where we do a lot with steam), the answer is dependent on if you're in a closed system or not. If I put some water in a closed container, it would evaporate only enough such that the gaseous water would reach the vapor pressure at that specific temperature. All temperatures above $\pu$ have a non-zero vapor pressure, so you could say that water evaporates at all temperatures, at least for a while, and then it will be in equilibrium with the liquid (or solid) state. However, if you are not in a closed system (say, outside with a cup of water), then the water will continue to evaporate to reach the vapor pressure, but the gas will continue to escape, so the water will never stop evaporating. The opposite, and the answer to your question, is also true. If you have circumstance when the surr...

By definition, the Boiling Point is the temperature at which the vapour pressure of the liquid equals the surrounding pressure, and the liquid turns into vapour. The phenomenon of boiling is pressure dependent and hence, the Boiling Point of a liquid may change depending upon the surrounding pressure. For example, due to the change in atmospheric pressure at different altitudes, water boils at 100°C (212°F) at sea level, but at 93.4°C (200.1°F), at 1,905 metres (6,250 ft). For a given pressure, different liquids will boil at different temperatures. Elevation in Boiling Point We know that pure water boils at 100°C at 1 atm pressure, but an interesting thing happens to the Boiling Point if we add a small amount of salt to that water. It has been experimentally proven that adding any form of non-volatile soluble to a liquid increases its Boiling Point. The amount by which the Boiling Point changes is directly proportional to the amount of soluble added. Let T 0 b denote the Boiling Point of a pure liquid, and T b denote the Boiling Point of a solution (solute + pure liquid). Then, \[ \Delta T_\] M = 115 gm/mol Interesting Facts • Did you know that if you climb a mountain, you’re going to find the Boiling Point there reduced? This is mainly because the higher the temperature, the more vapour you’re going to find! • You can boil water to use it as a disinfectant. Yes! This is because when you boil water, the microorganisms and bacteria get damaged due to its scalding heat, as a...