Can ypu boil water in 0 degrees centigrade if yes then how explain
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Answer:
Explanation:
Indeed you can. What actually happens is that any liquid or solid has a layer of its vapours surrounding it. This vapour imparts some pressure rather like the atmosphere imparts some pressure on its surroundings. This pressure is called vapour pressure. Now the liquid is in its state because its molecules have enough energy to move around however its vapour pressure is less than that of atmospheric pressure so atmosphere exerts a net force on it that keeps it in liquid state. It so happens that boiling point is the temperature when the vapour pressure is equal to atmospheric pressure and above that the vapour pressure is higher than the atmospheric pressure which means its vapours are free to go and more and more keep on leaving and as a result the liquid boils. Now if you get the pressure around the liquid down to its vapour pressure at 0 degrees then it will boil off at 0degrees. In fact if you keep it in space it will start boiling even as a solid at temperatures approaching absolute zero (-270degrees). Althoughboiling off from solid is known as sublimation. But in essence, yes it can happen.
1.6k views · View 6 Upvoters · Answer requested by Parmod Pandey
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Philip Howie
Philip Howie, materials scientist, academic, researcher
Answered Sep 23, 2015 · Upvoted by Gagan Srivastava, PhD Mechanical Engineering (Fluid Dynamics and Heat Transfer) · Author has 1.6k answers and 2.9m answer views
We can answer this question by looking at the equilibrium phase diagram for water:
Phase diagram of water
This shows the phase which is thermodynamically favourable at any given combination of temperature and pressure. If you look at the horizontal red line just above 100 kPa, you'll see how water behaves at (sea level) atmospheric pressure: it transitions from solid to liquid at 0°C and boils at 100°C.
Now look down to the triple point: the point at which solid, liquid and gas (vapour) are all in equilibrium. In fact, you'll see that the temperature is slightly higher (by 0.01°C) than the solid/liquid equilbrium temperature at atmospheric pressure. In other words, by the definition of the Celcius scale, it is NOT possible - the lowest temperature at which liquid and gas are ever in equilibrium is 0.01°C. In order to make the gas stable at a lower temperature, you need to further reduce the pressure, in which case it is not possible to find liquid water.
If you're willing to accept that as 'about' 0°C, then you can boil water by reducing the pressure below 611.73 Pa.
Note that the above applies to pure water; any impurities will shift the positions of each of the equilibrium lines on the phase diagram.
At boiling point, vapour pressure of the liquid = external (atmospheric) pressure