What is the difference between gas and vapour?

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Discussion Overview

The discussion centers around the differences between gas and vapor, exploring definitions, phase behavior, and the conditions under which each state exists. Participants examine theoretical and practical implications, including thermodynamic properties and examples from various substances.

Discussion Character

  • Debate/contested
  • Technical explanation
  • Conceptual clarification

Main Points Raised

  • Some participants propose that vapor refers to a state where a substance's gaseous phase is in equilibrium with its liquid or solid phases, typically below its boiling point.
  • Others argue that a gas is a single well-defined thermodynamic phase, while vapor is a mixture of gas and liquid phases, exemplified by clouds containing water vapor and steam being vaporized water.
  • A participant mentions that all vapors are gases, but not all gases are vapors, emphasizing that vapors can coexist with other phases below their critical points.
  • There is a discussion about the role of critical temperature in distinguishing between vapor and gas, with examples like water and oxygen provided to illustrate different critical points.
  • Some participants express confusion regarding the definitions, questioning whether certain gases can coexist with their liquid phases under specific conditions.
  • One participant asserts that visible steam is not steam but rather condensate, challenging the terminology used in the discussion.
  • Another participant notes that water vapor can exist in the atmosphere without being in equilibrium with its liquid or solid phases, highlighting the complexity of vapor behavior in real-world conditions.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the definitions and distinctions between gas and vapor. Multiple competing views remain, with some participants supporting traditional definitions while others challenge or refine them based on examples and theoretical considerations.

Contextual Notes

Some statements rely on specific definitions and assumptions that may not be universally accepted. The discussion reflects varying interpretations of phase behavior and terminology, particularly regarding the conditions under which gases and vapors coexist.

  • #31
Androgogue:

I sort of an aficionado of the so-called "New Steam", and one little trick is to use supercritical steam, but in such small amounts that safety hazards are reduced to a near nullity. I'm also much more interested in reciprocating plants than in turbines, as my primary interest is in railroad locomotives.

Seeing as this is getting a little off-topic, I'll start a new thread under "Mechanical Engineering". If you wish to continue this discussion, meet me there.
 
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  • #32
Andragogue said:
Saturated steam is the steam taken directly off the top of the steam drum. It is at its boiling/condensing temperature at the given pressure. (You might even call it a dewpoint vapor.)

Superheated steam is defined simply as steam heated above its boiling/condensing temperature at a given pressure. To make it, you take the saturated steam and put in through additional tubes in the firebox to add the superheat. The steam's temperature and its enthalpy are both increased.

I'm kinda sort of aware of that. In fact, your description of a water-tube boiler fails to account for the fire-tube superheater boilers of the American-type locomotive:

Loco001.jpg


Andragogue said:
You can get useful power out of saturated steam. But you will obviously get more power out of an equal mass of superheated steam due to its higher enthalpy. Studying a steam table makes this apparent.

I know that. My question concerns the weight of any kind of condensing engine versus the power which can be extracted from LP exhaust, as my primary interest involves engines other than stationary.

Andragogue said:
However, if you remember the difference between sensible heat (the heat energy that would be extracted through dropping the temperature of superheated steam) and latent heat (the heat energy that would be extracted by condensing saturated steam), in other words, about 0.5 btu/lb-deg F vs. 970 btu/lb at one atmosphere, you get potentially MORE heat energy out of steam if you condense it as you use it. (Of course, the actual amounts vary with system pressure.)

I totally get that. But, when you're drawing that last possible energy from saturated steam, don't you begin to need pumps to get the exhaust to the condenser, and, from there, to the water reservoir? What is the weight of those pumps, and the expenditure of energy needed to operate them, compared to the horsepower extracted from limp steam? (Once again, my primary interest is in non-stationary engines.)

Andragogue said:
I've operated both kinds of systems in industrial plants. New power plants operate with supercritical steam; which in this case is superheated steam raised to very high pressure. The benefit, beyond the higher enthalpy of the working fluid, is that as long as supercritical pressure is maintained as the steam expands in the turbine, you need not worry about a phase change (i.e., liquids condensing.)

No problem there, as that sounds like the recipe for New Steam (as long as you limit the live steam in your system, no matter how high the pressure, to an amount easily containable by means of light-weight containment vessels).

Andragogue said:
As to the comment about calling things by whatever names you want to use, I thought that was the whole point of this exercise... ? It does make a difference, my friend.

What this thread has demonstrated to me is the extent to which nomenclatural confusion is blocking access to conceptual reality.

***

I've now launched my new thread entitled: "Welcome to the "New Steam"" in the Mechanical Engineering category, and I think it's best that, if you wish to continue this discussion, you post any response you may have there.
 

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