On Monday, April 16, 2018 at 12:19:15 AM UTC-7, Arindam Banerjee wrote:

I would say, that in outer space with no other molecules around to
push H2O molecules apart, the tendency for them to stick to form
ice would be more pronounced than on the Earth's surface.

At room temperature and zero pressure they would be above boiling temperature and would fly apart, and they would have nothing to
stick to in outer space.

I don't understand the concept of room temperature and zero pressure.
When pressure is zero (as in outer space) the temperature is zero so
far as the ambient is concerned given no sunlight, etc.

So how exactly can one have room temperature and zero pressure on Earth?

In an enclosed container, using a vacuum pump.

Taking out the air from a cavity thus reducing the pressure to say zero reduces the temperature of the cavity where the air existed.

Yes, you may have to heat it too.

P1V1/T1 = constant as per universal gas law

Making P1 tending to 0, keeping V1=V2, means T1 tending to 0 to maintain the gas law.

The room temperature is measured outside the cavity.

But all of this is academic. The point is that the isolation you postulated
doesn't take place under normal conditions.

All I am saying is that when a molecule of water evaporates, what does happen?

Must two or more molecules of water simultaneously evaporate and unite automatically to form a nanodroplet of water - and this, always?

or

Does a single molecule of water evaporate at room temperature and remain single until it finds another molecule or nanodroplet to unite with?

It is the first always. Never does the second happen under normal
ambient conditions.

To understand why this is *always* the case you would have to first
understand the polarity neutralization associated with H bonds. Only
if there are enough associated H bonds is polarity low enough to
allow the molecules associated with a nanodroplet to break free from
the surface of pooled water.

Strangely, the amount of force necessary to break one molecule of H2O
free from the surface of liquid water is much greater than that
associated with a nanodroplets. This is because the nanodroplet
can collectively have low polarity but the singular H2O molecule
can only have full polarity.

Be aware that H bonds alleviate or neutralize 25% of the polarity in
BOTH of the H2O molecules that participate in the bonds. When you
consider this fact and its implications you are starting to understand
why water has so many anomalies.

In the video I am about to release I will explain the quantum mechanics
that underlie this strange reality associated with hydrogen bonding
between H2O molecules.

I fully agree with you that under 100degC at NTP water has no business
to remain as a gas - it has to be water. However, what happens
in a closed space, as in the petrol can experiment I had talked about,
is not what happens in an open space.

The only difference an enclosed container brings is the ability to control pressure. IT DOES NOT EFFECT THE PROPERTIES OF H2O!!!

But here on earth, under normal atmospheric pressures at the surface and an
atmosphere that is saturated with H2O, even in the driest of dry environments, that would be impossible.

Dry air by definition has no H2O,

You are being picky for no good reason. Dry air in the troposphere
is never 100% dry. And it would not be able to remain hot in the
proximity of other air molecules. I suppose, possibly, at the top
of the troposphere where it really is dry and somewhat hot an H2O
molecule might be able to remain monomolecular. But that is academic.

I am not an academic. I am a practical engineer. I would say that
simulation of a very small space tracking the behaviour of
each and every molecule in it (coming and going from the space,
and uniting or repelling therein) would give a fair clue
about the way water molecules behave in air. You can have
your nanodroplets there, or a mixture of nanodroplets and
individual molecules.

This simulation approach, I found very useful to model complex call
centre networks. The recommndations made as a result had a lot of
backing from the most fundamental positions.

The confounding factor for any such simulation is the fact that it is
just about impossible to reliably determined the size of the
nanodroplets. This problem has confounded researchers going back 200 years.

So this simulation, if made good enough, will provide proper
predictions with respect to humidity.

With further improvements, it could lead to developments relating to
cloud seeding, creation of rain, etc. and that would be a great boon
for dry countries.

Understanding the genuine behavior of H2O will be a boon to all of the
natural sciences--sciences that are currently handicapped by our
absurdly simplistic understanding of H2O that has been foisted upon us
by an academic tradition that is greedily provides artificially
simplistic models/explanations of H2O and hydrogen bonding (between
water molecules) to a public that is thirsty for simple models.

so a single molecule of H2O will find no other molecule of H2O
with which to stick. If there are other molecules then sticking
to form multimolecules will become a random issue involving the
chances of collision. I just don't get the impossibility part,
unless you are holding that as soon as 100degC steam is released
into dry air, all the monomolecules MUST unite to form
multimolecules. ALL of them.

Yes, they reform into multimolecules almost instantly, just as
soon as they cool below 100C.

If you say so. I would like your assertion to be based upon
simulation as I described above. How the 100deg water molecules
would move (faster than say at 10deg) and what chaces they have of
uniting in a volume where they are released.

I don't disagree, and that is why I am producing the video I am
about to release.

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