What is the state of hydrogen fluoride at 0.3 MPa?
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I would like to ask the experts: at 0.3 MPa, is hydrogen fluoride in a gas-liquid mixture? The temperature is room temperature, and can this pressure be achieved solely through vaporization? I did the calculations: at 0.3 MPa, the boiling point of hydrogen fluoride is 58 degrees. This means that at room temperature its vapor pressure cannot reach 0.3 MPa. What I’m interested in now is whether this pressure of 0.3 MPa can be achieved by applying external nitrogen pressure or through spontaneous evaporation. Which expert is familiar with this topic? Please help me out; it would be great if you could explain it to me, as I find myself a bit confused about it.
Is there hydrogen fluoride gas inside?
Does its pressure need to be provided by external nitrogen pressure, or can it be achieved through evaporation?
The data I simulated shows that the boiling point is 64°C at 0.3 MPa; therefore, at room temperature and 0.3 MPa, it is in liquid form (the boiling point at standard pressure is 20°C). If a pressure of 0.3 MPa is required for the liquid, then either nitrogen compression as mentioned by the poster or raising the temperature can be used; it is not possible to achieve 0.3 MPa through gas-liquid equilibrium at room temperature. However, if a pressure of 0.3 MPa is required for the gas, then heating to cause vaporization or the use of a compressor is necessary, and the temperature must be above 64°C. Please don’t criticize if there are mistakes; that’s my understanding.
The boiling point of liquid hydrogen fluoride is around less than 20 degrees, but its melting point is very low.
My understanding is similar to yours. I have a hydrogen fluoride storage tank here, at 0.3 MPa, and no heating facilities are provided (in my view, the pressure remains at atmospheric levels). I asked the owner yesterday, and they said that the pressure is generated through the vaporization of hydrogen fluoride itself; their explanation is that its boiling point is 20 degrees, so it vaporizes easily at room temperature. But I always feel something is off – at normal pressure its boiling point is 20 degrees, allowing it to vaporize by absorbing heat from the atmosphere; however, at 0.3 MPa its boiling point is 60 degrees, so it shouldn’t be able to vaporize by absorbing heat from the air. I hope you can help me analyze it. Thank you
Then it’s possible that there are other inert gases present; at room temperature, the partial pressure of hydrogen fluoride does not reach 0.3 MPa, but the total pressure does reach 0.3 MPa.