I suppose it would bubble and boil making the meniscus indistinguishable from the meniscus of water boiling, it would eventually turn into a gas. When it's a gas you wouldn't wanna be nearby as mercury fucks with your nervous system.
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What happens if one tries to boil mecury?
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I suppose it would bubble and boil making the meniscus indistinguishable from the meniscus of water boiling, it would eventually turn into a gas. When it's a gas you wouldn't wanna be nearby as mercury fucks with your nervous system.
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It will produce mercury (II) oxide (solid form) and some heat. But you need to go up to 350 degrees Celsius.
I think.
Why would you do that anyway? Is it for photography?
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Why would it form a solid? It is a metal so it has to be cool to be a solid, at room temperature it's too hard to be a solid... I think
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Its solid under -28°Celcius.
Don't know that,Is mercury(II) oxide solid??Could be,don't know that...
Realy dont breath the fumes!
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mercury is the only D-Block metal to be a liquid at room temperature, when it boils I assume it would just turn into a gas. What else is likely to happen?
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I am sure you end up having mercury (II) oxide at the end in solid form. Do the equation.
As to the length of time, I ain't got a clue. Perhaps you get a gas and the red oxide after, but I... I don't know.
Wasn't it -38?
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i think it would boil and then turn into gas like these people said...
but it does fuck with your nervous system... i had some in my hand once... it was liquidy...
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Mercury is fun to play with, it's really weird stuff.
It's only really dangerous if it's taken into the body (IE inhaled or seeps into a wound)
If you have enough mercury, fill a container full of it and look at the meniscus and compare it to water.
Could mercury be used a fuel of some kind? does it burn or react with another element?
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it wouldnt turn into mercury (II) oxide becuase he wants to boil it not burn it. It needs to be about 350 degrees C for it to boil I think.
I don't think mercury reacts with another element to produce sufficient heat for it to be used as a fuel, but hey i could be wrong.
my physics teacher froze mercury he was very happy about this accomplishment and wasted an hour explaining it,,,
Strictly speaking, if we were just interested in the boiling properties of this element, where the oxidation-reduction reaction were of little consequence, then it would vaporize at 357 degrees Celsius (630 K), under standard conditions. Its melting point lies at -38.7 degrees Celsius (234.5 K). Which is why this metallic element exists as a liquid at STP. The only other element to act in this manner is bromine, which is nonmetallic. Here is a table of the the physical properties of quicksilver..
However, Solace does raise an interesting question. What really happens to this species if it were to sit at room temperature in a flask, and then it were to be heated? At STP elemental mercury will oxidize to form some mercury (II) oxide, a mercuric compound. We don't here much about mercurous compounds because they are pretty unstable and easily decompose into elemental mercury.
Solace proposed that mercury will react with oxygen near its boiling point to produce the mercuric oxide in a reaction similar to the following:
Hg + 1/2 O(2) -----> HgO
To determine if this is true we must look to thermodynamic properties to predict the behavior at various temperatures.
Let's set up the following tables at standard temperature and pressure:
Heat of enthalpy of Formation (kJ/mol) - del(Hf)
HgO -90.7
Hg 0 (elemental)
O(2) 0 (elemental)
Gibb's Free Energy of Formation (kJ/mol) - del(Gf)
HgO -58.5
Hg 0 (elemental)
O 0 (elemental)
Absolute Entropy (J/(K*mol)) - del(S)
HgO 72.0
Hg(l) 77.4
O 205.0
We know by looking at the Gibb's free energy, whose sign is negative, that the reaction will proceed spontaneously in the forward direction. But alas, these data are for temperatures at 25 deg C. To determine how fast it would react at this temperature we would need to look at the reaction kinetics. We will reserve that discussion for another day.
From Thermodynamics, we know that we can predict the behavior over a range of temperatures by looking at the standard enthalpies of reaction and standard entropies of reaction to predict the sign of the Gibbs free energy over a range of temperatures, according to the relationship known by the second law of thermodynamics:
del(G)rxn = del(H)rxn - [T*del(S)rxn]
we also know that:
del(H)rxn = [the sum of the stoichiometric coefficients of the products * heats of formation of the products] - [the sum of the stoichiometric coefficients of the reactants * heat of formation of the reactants]
and that
del(S)rxn = [the sum of the stoichiometric coefficients of the products * absolute entropies of the products] - [the sum of the stoichiometric coefficients of the reactants * absolute entropies of the reactants]
Using the table to calculate values for the forward reaction we get
del(H)rxn = (-90.7)-(0+0) = -90.7
and
del(S)rxn = (72)-(.5(205)+77.4) = -107.9
If we were to run the reaction in reverse, we would get the same values with opposite signs.
According to the Gibbs 2nd law relation, we can tell that for systems with both del(H)rxn and del(S)rxn negative that the reaction will proceed spontaneously at low temperatures, while at high temperatures the reverse reaction is favored, and visa versa for a system where both signs are positive values.
This demonstration in the second law shows that it would be highly unlikely for mercury(II) oxide to exist around the boiling point of elemental mercury. In reality, the decomposition reaction is favored:
HgO ----------> 1/2 O(2) + Hg
That is to say even if mercuric oxide were to form at the lower temperatures it would decompose by the time it got to the boiling temperature of elemental mercury. In any case, you would be wise to boil your mercury under a very powerful hood because gaseous mercury is extremely toxic and reactive with your body chemistry, and that is precisely what would be present in the air.
